3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The same amount of MgCl, is added as previously and the total volume of EDTA solution required is 22.44 mL. d) Assume all of the Ca* in the water comes from CACO3. moles of CaCO, are in 1 L of water? How many moles How many grams of CaCO, are in 1 L of water? grams

3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The same amount of MgCl, is added as previously and the total volume of EDTA solution required is 22.44 mL. d) Assume all of the Ca* in the water comes from CACO3. moles of CaCO, are in 1 L of water? How many moles How many grams of CaCO, are in 1 L of water? grams

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 100 mL sample of a 0.300 M solution of a weak monoprotic acid is titrated with 0.150 M KOH. After 100 mL of the KOH solution is added, the pH is 5.24. What will be the pH after another 100 mL of the KOH solution is added? A. 8.82 B. 10.48 C. 8.62 D. 9.12 E. 9.01
3. a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO, and an 0.68 M solution of NAOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. b. If the acid used in a. was nitric acid, HNO, could the same buffer solution be made? Briefly explain. If the buffer solution prepared in a. also contained ~10°M Ni²* and ~10-6 M Pb²* , could those metal ions be separated from each other by saturating the solution with H,S? Explain your answer by showing the necessary calculations. C.
Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
A sample of antacid tablet that contains NaHCO3 is analyzed in the lab. The student dissolves 1.50g tablet in 35.0 mL of HCl solution containing 0.0300 mole of HCl. The back-titration of the excess HCl require 10.5 mL of 2.05M NaOH solution. 1) If that tablet label showed that each tablet contains 0.950 gram of NaHCO3. Determine the percent error in the student experiment. 2) Calculate the mass percent of the NaHCO3 in the tablet.
3. A 0.3535 g sample of KHP requires 19.27 mL of NaOH to reach the end point. What is the concentration of NaOH? 4. What properties should the indicator have for titration of KHP with NaOH?
A 1 liter solution contains 0.427 M hydrofluoric acid and 0.569 M sodium fluoride.Addition of 0.213 moles of potassium hydroxide will:(Assume that the volume does not change upon the addition of potassium hydroxide.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
A 1 liter solution contains 0.567 M acetic acid and 0.425 M potassium acetate.Addition of 0.213 moles of nitric acid will:(Assume that the volume does not change upon the addition of nitric acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
0.5 M of stock solution is given to be used for Titrant 1. Titrant 2 is going to be created by diluting 0.5 M stock solution to 0.1 M. How much stock solution (volume) will be needed to create 25 mL of the 0.1 M Titrant solution.
A 1 liter solution contains 0.324 M acetic acid and 0.243 M potassium acetate.Addition of 0.122 moles of hydrobromic acid will:(Assume that the volume does not change upon the addition of hydrobromic acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water. 2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH;*(aq) + Before (mol) Change (mol) After (mol) 5 RESET 0.200 0.100 +x 0.200 + x 0.200 - x -x 0.100 + x 0.100 - x 1.00 x 103 -1.00 x 10-3 2.00 x 10-3 -2.00 x 10-3 6.00 x 103 -6.00 x 10-3 7.00 x 10-3 -7.00 x 103 8.00 x 103 -8.00 x 103