Determine the pH change when 0.079 mol HI is added to 1.00 L of a buffer solution that is 0.372 M in HF and 0.382 M in F.pH after addition - pH before addition = pH change Determine the pH change when 0.079 mol HI is added to 1.00 L of a buffer solution that is 0.372 M in HF and 0.382 M in F.pH after addition - pH before addition = pH change

The objective of the question is to calculate the change.

Answered: Determine the pH change when 0.079 mol…

Determine the pH change when 0.079 mol HI is added to 1.00 L of a buffer solution that is 0.372 M in HF and 0.382 M in F pH after addition - pH before addition = pH change =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 15QAP: A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of...

See similar textbooks

Related questions

Q: 13. Calculate the [H+] in a 0.15 M Ba(NO3)2 solution.

A: A salt of strong acid and strong base is always neutral in nature with its pH is always equal to 7…

Q: The pKa of the weak acid HA is 4.49. If 0.17 mL of a 1.00 M solution of hydrochloric acid are added…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: A pharmacist adds 30 mL of a 6% (w/v) sodium bicarbonate injection to 357 mL of a 5% (w/v) dextrose…

A: In this pharmaceutical scenario, a pharmacist is tasked with preparing a solution by combining two…

Q: 7.50 g of a certain Compound x, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: The mass of the Compound X is 7.50 g.The molecular mass of the compound X is 150 g/mol.The mass of…

Q: When Zn metal was dipped in a solution of acid, it released hydrogen gas. This reaction can be…

A: Oxidation is defined as increase in oxidation state of the element.It can also be defined as…

Q: 4.) Please draw the mechanisms and products of these reactions. Indicate stereochemistry where…

A: 4a. Halohydrin formation reaction. 4b. Hydrohalogenation reaction.

Q: 7. Which reaction would occur faster and why? A. 1. CI II. O CI CH3S CH3S S- S-

A: The rate of a reaction is related to various factors including the nature and stability of the…

Q: A buffer solution is 0.412 M in H₂S and 0.236 M in NaHS. If Ka1 for H₂S is 1.0 × 10-7, what is the…

Q: Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the…

A: In an electrochemical cell, the chemical energy due to the chemical reactions is converted into…

Q: The fuel has a chemical formula of CH4 with 15% excess air. Find the actual mass of air in kg per…

A: Given,chemical formula of the fuel =CH4percentage of excess air = 15%we need to find the actual…

Q: Check the box under each structure in the table that is an enantiomer of the molecule shown below.…

A: Enantiomers are isomers that are non-superimposable mirror images of each other and have exact…

Q: Problem 9.63 Part A 190 mL of 0.30 M acetic acid, CH3 CO₂H Express your answer using two significant…

A: Given,A. Molarity of CH3CO2H = 0.30 M volume of CH3CO2H = 190 mLB. Molarity of NaOH = 0.23 M…

Q: Draw structural formulas for an aldehyde or ketone and alkyl (or aryl) bromide that could be used in…

Q: A reaction converts reactant X into product Y. It takes 6 minutes for the concentration of the…

A: Average rate of the reaction is calculated as follows: Average rate of reaction =…

Q: ОН ОН racemic racemic

A: Given are organic synthesis reactions.Both reactions have three step.Let's see reagents for each…

Q: which Com the conjugate addition of 10 NC D CN

A: The objective of the question is to give the product of the given reaction.

Q: 1. Predict the major product of each reaction, and state by which mechanism (S2, E2, SN1, or -schl…

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: An aqueous solution contains 0.26 M ammonium iodide. One liter of this solution could be converted…

Q: What would be the pH of a/solution made by adding 100.00 mL of 0.100 M NaOH to 100.0 mL of 0.100 M…

Q: What is the molarity of a solution made by dissolving 150.0 grams of K O H (MW = 56.12 g/mol) into…

A: Mass of KOH=150.0gMW of KOH=56.12g/molvolume of the solution=1.00Lmolarity of a solution=?

Q: For the reaction A (g) → 2 B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298…

Q: Can you show me how the mechanism is done? 1. 3 BH3 THF 2.3.3 NaOH, 3H2O

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: Using the arrow-pushing formalism, propose a mechanism to show the flow of electrons during the…

A: Epoxide undergo ring opening in presence of acid and a nucleophile through SN1 pathway.

Q: How would the substitution reaction shown affect the configuration of the substrate? Select one:…

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: How much heat is necessary to melt 12.8 g of solid gold? The heat of fusion of gold is 15.3 cal/g.

A: The objective of the question is to calculate the amount of heat required to melt 12.8 g of solid…

Q: A buffer solution that is 0.372 M in HF and 0.372 M in NaF has a pH of 3.14. Addition of which of…

A: Concentration of HF = 0.372 MConcentration of NaF = 0.372 MAs the concentration of acid, HF, is…

Q: Classify the p and d orbital diagrams based on whether they obey or violate Hund's rule. Obey 1 1 1…

A: Hund's rule statement Every orbital in a sublevel is singly occupied before any orbital is doubly…

Q: [Review Topics [References] Use the References to access important values if needed for this…

A: Given,Molarity of manganese (II) nitrate = 0.0667 Mvolume of manganese (II) nitrate = 150 mLKsp of…

Q: 100.0 mL sample of 0.020 M NiCl2 and a 100.0 mL ample of 0.025 M NalO3 are combined at 298 K. You…

Q: Using the following reagents, convert the given starting material into the given product. Each…

A: PCC convert 2° alcohol into ketone.Alkyl halide reacts with a base to form alkene.Halogen reacts…

Q: Draw the major product of this reaction. Ignore inorganic byproducts and CO 1.03 2. Zn, HOAc Q

A: One of the important reactions of alkene is ozonolysis. In the ozonolysis reaction, the…

Q: What is the systematic name for the given compound? X₂ Br What is the common name for the given…

A: Find and name the longest continuous carbon chainIdentify and name the groups attached to this…

Q: An active air sampler was used to trap polyaromatic hydrocarbons (PAHS) in the air above the sea…

A: Flow rate = 10 L per minuteTime of airflow = 12 hoursVolume of hexane used for elution = 10…

Q: If 20.0 g of NaCl is added to 100.0 mL of water, what is the %(m/m) of the NaCl in solution? Hint:…

Q: Me H Pr Et H 'H propa etmili meth!

A: IUPAC nomenclature of organic compounds refers to the systematic approach taken for the nomenclature…

Q: Table 1: Gas Laws and Molar Volume of Ideal Gas Data Initial Temperature Item Measured mass of zinc…

A: The number of moles of a substance is the ratio of the mass of the substance to the molar mass of…

Q: NH₂OH H₂SO4

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: 4. What are all possible enol forms of the ketone in the box? ОН 1 O 1 and 3 O 1 and 2 O 1, 2 and 4…

A: The question is about enol forms.In enol, ene (double bond) and ol (alcohol) are in…

Q: Aqueous sulfuric acid (H₂SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous…

A: Mass of = 66.7 gMass of NaOH = 70. gMinimum mass of sulfuric acid left over after the reaction = ?

Q: Which two mechanisms show the correct movement of electrons and formation of the major and minor…

A: The two possible reactions of the given tertiary halide are SN1 and E1.Tertiary alkyl halides…

Q: Construct the octahedral crystal-field splitting diagram for the metal in each species. V(H₂O)³+ OD…

A: The objective of the question is to construct the octahеdral crystal fiеld splitting diagram.

Q: compound contains carbon, hydrogen, and chlorine. It has a molar mass of 127.00 g/mol. Analysis of a…

A: Given:The percentage of carbon in the compound = 37.83 %The percentage of hydrogen in the compound =…

Q: CH₂ +HI →→ ?? Whal law used Draw Majons miner

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: Tu Please don't provide the handwriting solution Water can decompose into H_(2) and O_(2) via…

A: The objective of this question is to determine the number of moles of hydrogen gas (H2) that can be…

Q: Determine the mass, in grams, of silver that forms when 58.6 mL of 0.0310 M AgNO3 reacts with excess…

A: Balanced chemical reaction equation is Mg(s) + 2AgNO3(aq) → Mg(NO3)2(aq) + 2 Ag(s)Given:Volume of…

Q: Could you explain why it undergoes SN2 more specifically, I didn't get why a good leaving group and…

A: A good leaving group and a strong nucleophile cause a 2°alkyl halide to undergo SN2.Nucleophile…

Q: Which of the following redox reactions do you expect to occur spontaneously in the reverse…

Q: R Please don't provide the handwriting solution 23.3 mol of CH4 and 23.3 mol O2 were reacted…

A: The objective of the question is to determine the amount of water that can be theoretically produced…

Q: . How would you distinguish between the following isomers using their IR spectra? ОН Една ОН

A: IR spectra is used to identify the functional groups of unknown compounds based on a comparison of…

Q: Select the proper VSEPR shape (no lone pairs included in the drawing) for HC₂S(O)IF2. 4. Ÿ A B C O

A: The VSEPR theory is used to predict the shape of the molecules by using the repulsions between bond…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Determine the pH change when 0.079 mol HI is added to 1.00 L of a buffer solution that is 0.372 M in HF and 0.382 M in F.
pH after addition - pH before addition = pH change

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: The main aim of the question

VIEW

Step 2: Calculating the pH change

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 42 images

SEE SOLUTION Check out a sample Q&A here

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

A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
A buffer solution was prepared by adding 4.95 g sodium acetate to 250. mL of 0.150-M acetic acid. What ions and molecules are present in the solution? List them in order of decreasing concentration. Calculate the pH of the buffer solution. Calculate the pH of 100. mL of the buffer solution if you add 80. mg NaOH. (Assume negligible change in volume.) Write a net ionic equation for the reaction that occurs to change the pH.
A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL of the buffer. (b) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL pure (pH 7.00) water.
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?