Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Three buffers are prepared with equal concentrations of formic acid and sodium formate (Buffer 1), hydrofluoric acid and sodium fluoride (Buffer 2), and acetic acid and sodium acetate (Buffer 3). Rank the three buffers from highest to lowest pH at which they can buffer a solution (i.e., their buffering pH).(a) 1, 2, 3(b) 3, 2, 1(c) 2, 1, 3(d) 3, 1, 2
Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?arrow_forwardA buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?arrow_forwardA buffer contains 0.10 mol of acetic acid and 0.13 mol ofsodium acetate in 1.00 L. (a) What is the pH of this buffer?(b) What is the pH of the buffer after the addition of 0.02mol of KOH? (c) What is the pH of the buffer after the additionof 0.02 mol of HNO3?arrow_forward
- A buffer contains 0.20 mol of propionic acid (C2H5COOH) and 0.18 mol of sodium propionate (C2H5COONa) in 1.20 L. A. What is the pH of this buffer? B. What is the pH of the buffer after the addition of 0.01 mol of NaOH? C. What is the pH of the buffer after the addition of 0.01 mol of HI?arrow_forward25.00 mL of a 1.000 x 10-1 M solution of HClO4 is titrated with a 1.052 x 10-1 M solution of NH3. 1) What is the pH after 15.00 mL of NH3 solution has been added? 2) What is the pH after 35.00 mL of NH3 solution has been added? 3) What is the pH at the equivalence point? 4) What is one best indicator for this titration? 5) What is the best buffer pH for this titration?arrow_forwardAn industrial chemist studying bleaching and sterilizing pre-pares several hypochlorite buffers. Find the pH of (a) 0.100 M HClO and 0.100 M NaClO; (b) 0.100 M HClO and 0.150 M NaClO; (c) 0.150 M HClO and 0.100 M NaClO; (d) 1.0 L of the solution in part (a) after 0.0050 mol of NaOH has been added.arrow_forward
- What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric acid/fluoride buffer with a pH of 4.25 from 1.25 M HF and solid potassium fluoride? The Ka for HF is 6.8×10–4.arrow_forwardA buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 5.140. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.110 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2). What is the mass for oxalic acid dihydrate and disodium oxalate.arrow_forwardA buffer is prepared to contain 1.00 M acetic acid and 2.00 M sodium acetate. What is its pH? The Ka of acetic acid is 1.77 x 10^(-5). 1. pH 2. [OH-] 3. Numerator of the molar ratio between the acid and conjugate acid 4. Denominator of the molar ratio between the acid and conjugate acid 5. pKa 6. [H+] Here are the possible answers for each problem: 4.75 1.00 M acetic acid 2.00 M sodium acetate 5.05 8.91 x 10^(-6) [8.91 x 10^(-6)] 8.95 1.12 x 10^(-9) [1.12 x 10^(-9)] No answer pHarrow_forward
- A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 4.718. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.251 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2).arrow_forward1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that contains 0.100 M HNO2 and 0.200 M NaNO2. How many moles of HNO2 and NaNO2 remain in solution after addition of the HCl? HNO2 = NaNO2 =arrow_forwardConsider the titration of 30.0 mL of 0.269 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. A) What is the pH of the solution before any acid has been added? B)What would be the pH of the solution after the addition of 20.0 mL of HI? C)How many mL of the HI would be required to reach the halfway point? D) What is the pH of the solution at the equivalence point? E) What would be the pH of the solution after the addition of 100.0 mL of HI?arrow_forward
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