Phosphoric acid is a triprotic acid ($K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, K_{a3} = 4.8 \times 10^{-13}$). To find the pH of a buffer composed of $H_2PO_4^- (aq)$ and $HPO_4^{2-} (aq)$, which $pK_a$ value should be used in the Henderson-Hasselbalch equation? - $pK_{a1} = 2.16$ - $pK_{a2} = 7.21$ - $pK_{a3} = 12.32$ Calculate the pH of a buffer solution obtained by dissolving 10.0 g of $KH_2PO_4 (s)$ and 25.0 g of $Na_2HPO_4 (s)$ in water and then diluting to 1.00 L. pH = \_\_\_\_

Phosphoric acid is a triprotic acid ($K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, K_{a3} = 4.8 \times 10^{-13}$). To find the pH of a buffer composed of $H_2PO_4^- (aq)$ and $HPO_4^{2-} (aq)$, which $pK_a$ value should be used in the Henderson-Hasselbalch equation? - $pK_{a1} = 2.16$ - $pK_{a2} = 7.21$ - $pK_{a3} = 12.32$ Calculate the pH of a buffer solution obtained by dissolving 10.0 g of $KH_2PO_4 (s)$ and 25.0 g of $Na_2HPO_4 (s)$ in water and then diluting to 1.00 L. pH = \_\_\_\_

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...

See similar textbooks

Similar questions

part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What would be the pH of this solution? part b: How many milliliters (mL) of 19.00 M NaOH are need to adjust the pH of this buffer to pH 10.00? Please answer part b
A buffered solution containing dissolved aniline, CH,NH,, and aniline hydrochloride, CH, NH, Cl, has a pH of 5.27. Determine the concentration of CH, NH in the solution if the concentration of CH, NH, is 0.275 M. The pK, of aniline is $ 9.13. [CH_NH] = = Calculate the change in pH of the solution, ApH, if 0.386 g NaOH is added to the buffer for a final volume of 1.35 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M
12:04 Question 4 of 9 Submit A buffer solution contains dissolved C6H5NH2 and C6H;NH;CI. The initial concentration of C6HŞNH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6HŞNH3* in the solution. The value of Kb for C6H;NH2 is 3.8 × 10-1º. 1 2 3 Let x represent the original concentration of C6H,NH,* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H5NH2(at H20(1) = OH-(aq) +C6H5NH3*(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.50 - 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 x 10-10 -1.6 x 10-10 3.8 x 10-10 -3.8 x 10-10 x + 4.20 x - 4.20 x + 6.3 x 10-5 х - 6.3 х 10-6 x + 1.6 x 10-10 x - 1.6 x 10-10 x + 3.8 x 10-10 x - 3.8 x 10-10 Tap here or pull up for additional resources
Be sure to answer all parts.What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.16 M C6H5COOH and 0.46 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures.[H3O+] = _____pH = ______
Q3
What is the hydroxide ion concentration in a solution that containing 0.50 mole of ammonium hydroxide and 0.05 mole of ammonium chloride per liter of solution? Since the pKb of ammonium hydroxide is 4.75? and What is the type of buffer solution? a- 1. 54 x 10-4 M. basic buffer b- 1.77 x 10-4 M. acidic buffer c- 1.77 x 10-4 M. basic buffer d- 1. 54x 10-4 M. acidic buffer الاختيارات b a O C d O
what volume of Boric acid 0.1 M and what volume of sodium hydroxide 0.1 M should be added together to produce a solution (buffer) with a pH of 9.1? (ka=6.0*10-10) 4H3BO3 +2NaOH --> Na2B4O7 +7H2O
You are titrating 30 mL of 0.100M H3PO4 with 0.200 M KOH. For H3PO4: Ka1=1.1X 10-², Ka2 = 7.5 X 10-8, and Ka3 = 4.8 X 10-¹3. What is the pH after you add 35.00 mL of KOH?
Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find the pH of a buffer composed of H2PO4−(aq) and HPO2−4(aq), which pKa value would you use in the Henderson–Hasselbalch equation? 1. p?a1=2.16 2. p?a2=7.21 3. p?a3=12.32 Calculate the pH of a buffer solution obtained by dissolving 21.021.0 g KH2PO4(s) and 39.0 g Na2HPO4(s) in water and then diluting to 1.00 L. pH=?
Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K of pyridine is 1.7 x 10-⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution pH at the equivalence point? (Two decimal places) Type your answer...
What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____
Question 4 a) Determine the pH of 0.10 M NAOH solution. b) Find out the pH of a 0.002 M acetic acid solution if it is 2.3% ionised at this dilution. c) A chemistry student desires to prepare one litre of a solution buffered at pH 9.00. How many grams of ammonium chloride haye to be added to one litre of 0.20 M NH3 to makesuch a buffer. pKb value of ammonia is 4.75 in the equation. NH3 + H20 = NH + OH