General, Organic, and Biological Chemistry
7th Edition
ISBN: 9781285853918
Author: H. Stephen Stoker
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 10, Problem 10.64EP
Write a balanced molecular equation for the preparation of each of the following salts, using an acid–base neutralization reaction.
- a. LiNO3 (lithium nitrate)
- b. BaCl2 (barium chloride)
- c. K3PO4 (potassium phosphate)
- d. Na2SO4 (sodium sulfate)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Determine the weight/volume of the chemicals needed to prepare the following solutions:
a) 100 ml of 0.9% (w/v) saline (NaCl)
b) 30 ml of 50% glycerol (v/v)
c) Electrophoresis requires TAE, which is a specific mixture of Tris base, acetic acid, and EDTA. TAE is normally made as a 50X concentrated stock. Provide a recipe to make 40 ml of 50X TAE.
The recipe for one liter of 50X TAE is as follows: 242g Tris base, 57.1 ml glacial acetic acid, 100 ml 0.5 M EDTA
Potentiometric titration curve is given below, which is obtained during the potentiometric
titration
between strong base KOH (0.2 M) with strong acid HI, label the point in the curve from the
following options.
If more than one points are present than write as x, y(means separate by using comma)
a)The point where pH is because of excess OH - ions.
b) The point where pH is only because of HI in water.
c)The point where [HI]= [I] in water.
d)The point where pH=pka
e) The point where all HI is neutralized.
f) The point where pH corresponds to solution of [I- ] in water.
14
13
12
11
10
9
pH
6.
TITIT TIT
Glycine hydrochloride (Cl− H3N+CH2COOH) is a diprotic acid that contains a carboxylic acid group and an ammonium group and is therefore called an amino acid. It is often used in biochemical buffers. Solve, In analogy with Figure , sketch the titration curve of this diprotic acid.
Chapter 10 Solutions
General, Organic, and Biological Chemistry
Ch. 10.1 - In an Arrhenius acidbase theory context, the...Ch. 10.1 - In an Arrhenius acidbase theory context, the...Ch. 10.1 - Which of the following statements concerning...Ch. 10.2 - Prob. 1QQCh. 10.2 - For the chemical reaction N3 + H2O HN3 + OH, the...Ch. 10.2 - The chemical formula for the conjugate acid of ClO...Ch. 10.2 - Which of the following is a conjugate acidbase...Ch. 10.2 - Prob. 5QQCh. 10.3 - Which of the following is not a polyprotic acid?...Ch. 10.3 - For the triprotic acid H3PO4, the reactant in the...
Ch. 10.3 - Prob. 3QQCh. 10.4 - In which of the following pairs of acids are both...Ch. 10.4 - Prob. 2QQCh. 10.4 - Prob. 3QQCh. 10.5 - Acid ionization constants give information about...Ch. 10.5 - Prob. 2QQCh. 10.5 - Which of the following is the strongest acid? a....Ch. 10.5 - Prob. 4QQCh. 10.6 - Which of the following is an inappropriate...Ch. 10.6 - Prob. 2QQCh. 10.6 - In which of the following pairs of substances are...Ch. 10.7 - Prob. 1QQCh. 10.7 - Prob. 2QQCh. 10.7 - Prob. 3QQCh. 10.8 - Prob. 1QQCh. 10.8 - Prob. 2QQCh. 10.8 - What is the [OH] in an aqueous solution in which...Ch. 10.8 - Prob. 4QQCh. 10.8 - Prob. 5QQCh. 10.9 - Prob. 1QQCh. 10.9 - Prob. 2QQCh. 10.9 - Prob. 3QQCh. 10.9 - A solution with a pH of 12.0 is a. weakly acid b....Ch. 10.9 - Prob. 5QQCh. 10.9 - If the pH of a solution increases from 4.0 to 6.0...Ch. 10.9 - Prob. 7QQCh. 10.10 - Prob. 1QQCh. 10.10 - Prob. 2QQCh. 10.11 - Prob. 1QQCh. 10.11 - Prob. 2QQCh. 10.11 - Prob. 3QQCh. 10.12 - Which of the following combinations of substances...Ch. 10.12 - Prob. 2QQCh. 10.12 - Prob. 3QQCh. 10.12 - The chemical reaction that occurs when a HCN/CN...Ch. 10.13 - Prob. 1QQCh. 10.13 - For a buffer where the acid and conjugate base are...Ch. 10.14 - Which of the following statements concerning...Ch. 10.14 - In which of the following pairs of compounds are...Ch. 10.14 - Prob. 3QQCh. 10.15 - How many equivalents of Ca2+ ion are present in a...Ch. 10.15 - Prob. 2QQCh. 10.15 - Prob. 3QQCh. 10.15 - Prob. 4QQCh. 10.16 - Determining the concentration of an acid using an...Ch. 10.16 - Prob. 2QQCh. 10.16 - Prob. 3QQCh. 10 - In Arrhenius acidbase theory, what ion is...Ch. 10 - What term is used to describe the formation of...Ch. 10 - Classify each of the following as a property of an...Ch. 10 - Classify each of the following as a property of an...Ch. 10 - Write equations depicting the behavior of the...Ch. 10 - Write equations depicting the behavior of the...Ch. 10 - Indicate whether the first listed reactant in each...Ch. 10 - Indicate whether the first listed reactant in each...Ch. 10 - Write chemical equations that show the indicated...Ch. 10 - Write chemical equations that show the indicated...Ch. 10 - Indicate whether or not the two members of each of...Ch. 10 - Indicate whether or not the two members of each of...Ch. 10 - Write the formula of each of the following. a....Ch. 10 - Write the formula of each of the following. a....Ch. 10 - Identify the conjugate acidbase pairs associated...Ch. 10 - Identify the conjugate acidbase pairs associated...Ch. 10 - The ion HCO3 is an amphiprotic ion. Write the...Ch. 10 - The ion HPO42 is an amphiprotic ion. Write the...Ch. 10 - Classify each of the following acids as...Ch. 10 - Classify each of the following acids as...Ch. 10 - Prob. 10.21EPCh. 10 - For each of the acids in Problem 10-19 indicate...Ch. 10 - Write chemical equations showing the individual...Ch. 10 - Write chemical equations showing the individual...Ch. 10 - Prob. 10.25EPCh. 10 - The formula for tartaric acid is preferably...Ch. 10 - Pyruvic acid, which is produced in metabolic...Ch. 10 - Oxaloacetic acid, which is produced in metabolic...Ch. 10 - Classify each of the acids in Problem 10-19 as a...Ch. 10 - Classify each of the acids in Problem 10-20 as a...Ch. 10 - For each of the following pairs of acids, indicate...Ch. 10 - For each of the following pairs of acids, indicate...Ch. 10 - For each of the following pairings of acid and...Ch. 10 - For each of the following pairings of acid and...Ch. 10 - The HCl in a 0.10 M HCl solution is 100%...Ch. 10 - The HNO3 in a 0.50 M HNO3 solution is 100%...Ch. 10 - The following four diagrams represent aqueous...Ch. 10 - Using the diagrams shown in Problem 10-37, which...Ch. 10 - Which of the terms weak, strong, monoprotic,...Ch. 10 - Which of the terms weak, strong, monoprotic,...Ch. 10 - Write the acid ionization constant expression for...Ch. 10 - Write the acid ionization constant expression for...Ch. 10 - Prob. 10.43EPCh. 10 - Write the base ionization constant expression for...Ch. 10 - Prob. 10.45EPCh. 10 - Using the acid ionization constant information...Ch. 10 - A 0.00300 M solution of an acid is 12% ionized....Ch. 10 - A 0.0500 M solution of a base is 7.5% ionized....Ch. 10 - Is the monoprotic acid Y or the monoprotic acid Z...Ch. 10 - Is the monoprotic acid Y or the monoprotic acid Z...Ch. 10 - Classify each of the following substances as an...Ch. 10 - Classify each of the following substances as an...Ch. 10 - Prob. 10.53EPCh. 10 - Indicate whether or not both members of each of...Ch. 10 - Prob. 10.55EPCh. 10 - Write a balanced equation for the dissociation...Ch. 10 - Indicate whether each of the following reactions...Ch. 10 - Indicate whether each of the following reactions...Ch. 10 - Without writing an equation, specify the molecular...Ch. 10 - Without writing an equation, specify the molecular...Ch. 10 - Write a balanced chemical equation to represent...Ch. 10 - Write a balanced chemical equation to represent...Ch. 10 - Prob. 10.63EPCh. 10 - Write a balanced molecular equation for the...Ch. 10 - Prob. 10.65EPCh. 10 - What is the molar hydronium ion concentration in...Ch. 10 - Indicate whether each of the solutions in Problem...Ch. 10 - Prob. 10.68EPCh. 10 - Prob. 10.69EPCh. 10 - Prob. 10.70EPCh. 10 - Prob. 10.71EPCh. 10 - Indicate whether each of the solutions in Problem...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - What is the [H3O+] value in solutions with each of...Ch. 10 - What is the [H3O+] value in solutions with each of...Ch. 10 - Prob. 10.81EPCh. 10 - What is the molar hydronium ion concentration in...Ch. 10 - Prob. 10.83EPCh. 10 - Indicate whether each of the following samples is...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Prob. 10.86EPCh. 10 - Consider the following four solutions: (1) apple...Ch. 10 - Consider the following four biological solutions:...Ch. 10 - For each of the following pairs of solutions,...Ch. 10 - Prob. 10.90EPCh. 10 - Calculate the pKa value for each of the following...Ch. 10 - Calculate the pKa value for each of the following...Ch. 10 - Acid A has a pKa value of 4.23, and acid B has a...Ch. 10 - Acid A has a pKa value of 5.71, and acid B has a...Ch. 10 - If a weak acid has a pKa value of 8.73, what is...Ch. 10 - If a weak acid has a pKa value of 7.21, what is...Ch. 10 - Classify each of the following salts as a strong...Ch. 10 - Classify each of the following salts as a strong...Ch. 10 - Prob. 10.99EPCh. 10 - Identify the ion (or ions) present in each of the...Ch. 10 - Prob. 10.101EPCh. 10 - Prob. 10.102EPCh. 10 - Both ions in the salt ammonium cyanide (NH4CN)...Ch. 10 - Both ions in the salt ammonium acetate (NH4C2H3O2)...Ch. 10 - Arrange the following 0.10 M aqueous solutions in...Ch. 10 - Arrange the following 0.10 M aqueous solutions in...Ch. 10 - Predict whether each of the following pairs of...Ch. 10 - Predict whether each of the following pairs of...Ch. 10 - Identify the two active species in each of the...Ch. 10 - Identify the two active species in each of the...Ch. 10 - Prob. 10.111EPCh. 10 - Write an equation for each of the following...Ch. 10 - Prob. 10.113EPCh. 10 - Prob. 10.114EPCh. 10 - Prob. 10.115EPCh. 10 - A buffer solution has a pH value of 9.8. Which...Ch. 10 - The following four diagrams represent aqueous...Ch. 10 - Using the diagrams shown in Problem 10-117, which...Ch. 10 - Identify the buffer system(s)the conjugate...Ch. 10 - Identify the buffer system(s)the conjugate...Ch. 10 - Prob. 10.121EPCh. 10 - Prob. 10.122EPCh. 10 - What is the pH of a buffer that is 0.230 M in a...Ch. 10 - What is the pH of a buffer that is 0.250 M in a...Ch. 10 - What is the pH of a buffer that is 0.150 M in a...Ch. 10 - What is the pH of a buffer that is 0.175 M in a...Ch. 10 - Classify each of the following compounds as a...Ch. 10 - Classify each of the following compounds as a...Ch. 10 - Indicate whether solutions of each of the...Ch. 10 - Indicate whether solutions of each of the...Ch. 10 - How many ions, per formula unit, are produced when...Ch. 10 - How many ions, per formula unit, are produced when...Ch. 10 - Write a balanced chemical equation for the...Ch. 10 - Prob. 10.134EPCh. 10 - Four different substances of the generalized...Ch. 10 - Which of the diagrams in Problem 10-135 represents...Ch. 10 - Indicate the number of equivalents in each of the...Ch. 10 - Indicate the number of equivalents in each of the...Ch. 10 - Indicate the number of equivalents in each of the...Ch. 10 - Indicate the number of equivalents in each of the...Ch. 10 - A solution contains 48 mEq of Ca2+ ion. Based on...Ch. 10 - Prob. 10.142EPCh. 10 - Prob. 10.143EPCh. 10 - A solution is 0.0030 M in H2PO4 ion. What is this...Ch. 10 - Prob. 10.145EPCh. 10 - Prob. 10.146EPCh. 10 - How many mEq of HCO3 are present in a solution...Ch. 10 - How many mEq of Ca2+ are present in a solution...Ch. 10 - Determine the molarity of a NaOH solution when...Ch. 10 - Determine the molarity of a KOH solution when each...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Consider a HCI solution with a pH of 4.70. a) Calculate the concentration of HCl. b) Identify the two underlying assumptions in part a). c) The original solution is diluted by 1,000 fold. Calculate the pH of the resulting solution. Make sure to indicate if the forementioned assumptions are still valid.arrow_forwardA 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. The other 50.00 mL remaining solution was also analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. e) Write the cell notation of the potentiometric set-up with SCE as the reference electrode. f) Write the Nernst equation that describes the indicator electrode set-up.arrow_forwardTrans-oleic acid (18:1,D9) has a melting temperature of (44.5C) and cis-oleic acid (18:1,D9) has a melting point of (13.4C). Briefly explain the difference in melting points between the two. tw.arrow_forward
- The glass electrode used in commercial pH meters gives an electrical response proportional to the concentration of hydrogen ion. To convert these responses to a pH reading, the electrode must be calibrated against standard solutions of known H+ concentration. Determine the weight in grams of sodium dihydrogen phosphate (NaH2PO4 · H2O; FW 138) and disodium hydrogen phosphate (Na2HPO4 ; FW 142) needed to prepare 1 L of a standard buffer at pH 7.00 with a total phosphate concentration of 0.100 M . See Problem 24 for the pKa values of phosphoric acid.arrow_forwardThe Ksp values of silver chromate Ag2CrO4 and silver iodate Ag(IO3) are given below. Ag2CrO4 Ag(IO3) Ksp 1.12 x 10-12 3.17 x 10-8 Based on these Ksp values, which of the following is true? Choose one option only. Options: a. In the solution consisting of 1.00 x10-4 M Ag+ and 5.00 x10-5 M CrO42-, Ag2CrO4 precipitate will form. b. In the solution consisting of 1.0 x10-4 M Ag+ and 1.0 x10-4 M IO3-, Ag(IO3) precipitate will form. c. In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3). d. In the solution consisting of 0.200 M CrO42- and 0.200 M IO3-, Ag2(CrO4) will precipitate first if we add Ag+ ions gradually into the above mixture.arrow_forwardThe ionization of p-nitrophenol is shown below (pKa = 7.0): a. Identify the weak acid and conjugate base. b. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? c. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms? d. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why? e. A solution of p-nitrophenol at pH 7.95 was found to have an A400 of 0.255 . What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 18,500 M-1cm-1 and the pKa is 7.arrow_forward
- Three buffers are made by combining a 1M solution of acetic acid and a 1M solution of sodium acetate in the ratios shown in the table below. Which of these statements is true regarding the prepared buffers? (Ka= 1.7x10-5) pH of buffer 1 < pH of buffer 2 < pH of buffer 3 pH of buffer 1 = pH of buffer 2 = pH of buffer 3 pH of buffer 1 > pH of buffer 2 > pH of buffer 3 pH of buffer 1 = pH of buffer 2 > pH of buffer 3 pH of buffer 1 > pH of buffer 2 = pH of buffer 3arrow_forwardThe main constituents in vinegar are water and ethanoic acid (CH3COOH). In order to determine the concentration of acid in homemade vinegar, a student titrated 25 cm3 of 001 M NaOH against the vinegar. The equation for the reaction is: CH3COOH(aq) + NaOH(aq) ® CH3COONa(aq) + H2O(l) The following titration results were obtained: Burette readings (cm3) Rough 1 2 Final burette reading 20.10 38.90 31.40 Initial burette reading 0.10 20.00 12.50 Volume of vinegar used 20.00 18.90 18.90 (a) What volume of vinegar should be used in the calculation? (b) What is the mole ratio of NaOH:CH3COOH? (c) Calculate the number of moles of alkali in 25 cm3 of NaOH solution used. (d) How many moles of acid were used in the titration? (e) Calculate the…arrow_forwardA patient’s treatment plan requires two IV solutions to be administered:20% magnesium sulfate, MgSO4, and 10% calcium chloride, CaCl2. Thenurse is concerned, MgSO4 and CaCl2 are listed as incompatible IVsolutions with the risk of solid precipitate formation (image shown toright). Write the chemical equation that predicts the products thatform when combining MgSO4 and CaCl2. Please use the providedsolubility chart to help you determine chemical phases.arrow_forward
- Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. for pH 6, α4 = 2,2 x 10-5arrow_forwardComplete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid K Κα PK relative strength a a ☐ x10 A B C 1.2 × 10 3. 10 4 ☐ 11.539 ×arrow_forwardConsider these compounds: A. PbBr, B. MnS C. Ag,CO3 D. AIPO, Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that magnesium fluoride is more soluble than and magnesium fluoride is less soluble than| It is not possible to determine whether magnesium fluoride is more or less soluble than by simply comparing Kgp values.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ENVIRONMENTAL POLLUTION; Author: 7activestudio;https://www.youtube.com/watch?v=oxtMFmDTv3Q;License: Standard YouTube License, CC-BY