Use the following data to determine the percent mass of C a CO3 in an antacid tablet. 1.076 grams of antacid tablet dissolved 24.22 ml of 0.750 M HCI used to dissolved the tablet 4.68 mL of 1.00 M N a OH for the back-titration To not type units with your answer.

Use the following data to determine the percent mass of C a CO3 in an antacid tablet. 1.076 grams of antacid tablet dissolved 24.22 ml of 0.750 M HCI used to dissolved the tablet 4.68 mL of 1.00 M N a OH for the back-titration To not type units with your answer.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 114CP

See similar textbooks

Related questions

Q: Complete the equation for the dissociation of the electrolyte AgNO, (aq). Omit water from the…

Q: A 0.8159 g sample of HCl was placed into a 50 mL volumetric flask and the sample was thoroughly…

A: Number of moles of HCl = given mass / molar mass = 0.8159 g /36.46 g/mole = 0.022 mole

Q: Which of the following acids is the WEAKEST electrolyte? O A. hydrochloric acid B. nitric acid O C.…

A: weak electrolytes are the electrolytes that ionise partially on dissociation or we can say that weak…

Q: 1.80 grams of an impure mixture containing sodium carbonate required 84.0 mL of 0.125 M H2SO4(aq)…

A: An impure mixture containing Na2CO3 whose percentage of mixture is to be determined.

Q: What volume in milliliters of 0.0160 M Ca(OH), is required to neutralize 75.0 mL of 0.0300 M HCI?

Q: An aqueous solution of hydrobromic acid is standardized by titration with a 0.119 M solution of…

A: The reaction between hydrobromic acid and barium hydroxide is neutralization reaction.

Q: What volume in mL of 0.025 M HBr solution is to be required to titrations 125mL of a 0.049 M NaOH…

A: As per the reaction, NaOH(aq) + HBr(aq) -> NaBr(aq)+H2O(I) we can see that 1 mole of HBr is…

Q: While performing a neutralization reaction, Ben added 21.94 mL of 0.172 M H2SO4 to 48.98 mL of 0.375…

A: Answer : 0.152 M is the concentration of OH-, in M, that is unreacted in the solution after the…

Q: A solution of 0.332 M KOH is used to titrate 16.0 mL of a 0.192 M H3PO4 solution. What volume, in…

Q: For the following acid-base neutralization: 2 HNO3 (aq) + Ca(OH)2 (aq) --> 2 H20 (1) + Ca(NO32 (aq)…

A: We are given Molarity and volume of acid and molariy of base, we have been asked the volume of base…

Q: Calculate the molarity of a sodium hydroxide(NaOH) solution that is titrated with 0.6887 g of oxalic…

A: Given: The mass of oxalic acid taken = 0.6887 g The volume of NaOH solution required to reach the…

Q: nges to this answer. What is the "equivalence point" in a titration? O The point at which the…

Q: ered items or incomplete statements is followed by answers or by completions of the statement. ered…

A: Question 27: The Quality coordinating office is the quality control department maintain and store…

Q: During a standardization procedure, 24.22 mL of a sodium hydroxide (NaOH) solution were required to…

Q: 37.50 mL of a diprotic acid solution, whose concentration is unknown, is titrated with 12.54 mL of…

A: Given that, Volume of diprotic acid V1 = 37.50 mL Concentration of diprotic acid M1 = ? Volume of…

Q: Part A A solution of 0.358 M KOH is used to titrate 13.5 mL of a 0.182 MHPO, solution. What volume,…

A: The given data contains, Molarity of KOH = 0.358 M. Molarity of H3PO4 = 0.182 M. Volume of…

Q: i volume (in mL) of 0.250 M HCI would be required to completely with 4.0 0 a of ALin the following…

A: The number of moles of aluminium can be calculated as, Now, as per the balanced chemical reaction,…

Q: What mass of FeSO4.(NH4)2SO4. 6H2O is present in a sample if it is titrated to its equivalence point…

A: Given: Volume of KMnO4 = 4.100 mL Concentration of KMnO4 = 0.100 N mass of FeSO4.(NH4)2SO4.…

Q: 25.00 mL of a diprotic acid solution, whose concentration is unknown, is titrated with 12.54 mL of…

A: Given data: Volume of diprotic acid = 25.00 mL Volume of NaOH = 12.54 mL Concentration or molarity…

Q: The titration of 25.00 mL of a sulphuric acid solution of an unknown concentration requires 31.22 mL…

A: The reaction in which an acid and a base react to produce salt and water is called as…

Q: Use the References to access important values if needed for this question. An aqueous solution of…

A: Given : molarity of Ba(OH)2= 0.186 M Volume of HCl solution = 20.3 mL And volume of Ba(OH)2 solution…

Q: An aqueous solution of hydroiodic acid is standardized by titration with a 0.171 M solution of…

A: Given : Concentration of barium hydroxide i.e Ba(OH)2 = 0.171 M Volume of Ba(OH)2 required = 23.1 mL…

Q: An excess amount of ZN (s) is added to 50 ml of 0.800 M HCl. What mass in grams?

Q: 42.1 mL of 1.41 M hydroiodic acid is added to 29.3 mL of barium hydroxide, and the resulting…

A: Reactions leading to the creation of neutral salts and water are regarded as neutralization…

Q: Given the mole ratio of HCl to NaOH is 1:1 in the balanced acid base reaction A 15.52mL sample of…

Q: For a product to be legally called "vinegar", it must contain at lest 5.0% by mass of acetic acid,…

A: Given: Mass of vinegar sample = 10.00 g Concentration of KOH = 0.1250 M And volume of KOH solution…

Q: Which of the given solutions is in the solid phase? A. Iodine solution B. Dental fillings (amalgam)…

A: A solid compound have a fixed shape and mass. A liquid compound does not have a fixed shape, it will…

Q: Calculate the volume of 0.734 M HNO, that can be neutralized by 52.2 mL of a 1.96 M KOH solution.…

A: Consider the given information is as follows; Volume of HNO3 VHNO3 = ? Molarity of HNO3 MHNO3 =…

Q: A 13.8 mL solution of 0.176 M phosphoric acid (ag) is to be titrated with 0.384 M sodium hydroxide…

A: The given data contains, Molarity of phosphoric acid = 0.176 M. Volume of phosphoric acid = 13.8 ml.…

Q: I have 26.06 mL of an unknown-concentration Mg(OH), (aq) solution. I find that, when I add 23.75 mL…

Q: Which data set, of the two graphed here, would you expectto observe from a titration like that shown…

A: A titration curve is a graphical representation of the pH of a solution.

Q: A 25.0-mL sample of a 2.14 M NAOH solution is titrated with a 1.25 M HCI solution. What will be the…

A: The given data contains, Volume of NaOH V1 = 25 ml. Molarity of NaOH M1 = 2.14 M. Volume of HCl V2 =…

Q: A 5.0 g impure sample of sodium carbonate was titrated with an acid. The sample utilized 31.55 ml of…

A: The relationship between normality and molarity of a substance follows: Normality = n × Molarity…

Q: What is the molarity of an HCI solution if 25.5 ml of 0.438 M NaOH is required to neutralize 0.0250…

A: The given neutralization reaction between HCl and NaOH is : The given data is : The volume of NaOH…

Q: What colour is the resulting solution when the universal indicator is added to water? What colour is…

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

A: The neutralisation reaction taking place is 2 HBr + Ca(OH)2 -----> CaBr2 + 2 H2O Hence from the…

Q: One commercial method used to peel potatoes is to soak them in a NaOH solution for a short time and…

A: Firstly, write the neutralization reaction of a strong acid with a strong base.…

Q: A 4.36-g sample of an unknown alkali metal hydroxide is dissolvedin 100.0 mL of water. An acid–base…

A: Acid-Base indicators are the weak acid or base indicator that usually dissociates in water to give…

Q: An aqueous solution of hydroiodic acid is standardized by titration with a 0.108 M solution of…

A: given :- molarity of Ba(OH)2 solution = 0.108 M volume of Ba(OH)2 solution = 21.8 mL volume of HI…

Q: 1. In a titration, a 20 ml sample of 0.3 N HCI is neutralized with 55 ml of NaOH. a) Write the…

A: "Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: The chloride ion content of a 250.0-mL seawater sample was titrated against 0.1102 M silver nitrate,…

A: The Chloride ions from the seawater are titrated against silver nitrate and the objective of the…

Q: What is the molarity of an HCI solution if 25.5 mL of 0.438 M NaOH is required to neutralize 0.0250…

A: For neutralization product of molarity and volume of acid must be equal to the product of molarity…

Q: Calculate the concentration of all 1ons present in 0.472 g AlCl, in 250.0 mL of solution. MAI?+ MCl-

Q: Q4) Use the following data to determine the percent mass of C a CO3 in an antacid tablet. 1.189…

A: 1.189 grams of antacid tablet is dissolved in 24.21 mL of 0.750 M HCl solution. The resulting…

Q: 1) What do we mean by titration? 2) What is the concept of redox titration? 3) What is the…

A: (1) Titration is a process in which, liquid amount of one substance determined by using another…

Q: In titration, one solution is added to another solution until a chemical reaction between the…

A: The balanced chemical equation for the reaction between the given acid and base is shown below.…

Q: pipette pipette filler A student uses the apparatus to determine the concentration of a solution of…

A: Correct Option : Titrant

Q: By titration it is found that 76.7 mL of .151 M NaOH(aq) is needed to neutralize 25.0mL. Calculate…

A: Given information: The volume of HCl is 25.0mL The concentration of NaOH is 0.151 M The volume of…

Q: Titration of a 25.00 mL sample of acid rain required 13.23 mL of 0.009567 M KOH to reach the end…

Q: (f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Use the following data to determine the percent mass of Ca CO3 in an antacid
tablet.
1.076 grams of antacid tablet dissolved
24.22 ml of 0.750 M HCI used to dissolved the tablet
4.68 mL of 1.00 M N a O H for the back-titration
To not type units with your answer.
Your Answer:

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

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

An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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.
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80105 as Ka for acetic acid. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?
Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
What acid-base indicators, shown in Figure 18.24 would be suitable for the neutralization reaction whose titration curve is shown in Figure 18.30?Why?