29. Determine the ph of a 0.50 M NaH2PO4 and 0.10 M N22HPO4 solution, pKa is7.21.A. 5,5O B. 6.5)C. 4,5OD.7.530. Determine the ph of a 0.30 M NaH2PO4 and 0.20 M H3PO4 solution. pka is2.16.O A. 1.3B. 2.3C. 3.3OD.4.3

The solution contains weak acid NaH2PO4 and its conjugate base Na2HPO4. So, this is a buffer…

29. Determine the ph of a 0.50 M NaH2PO4 and 0.10 M Na2HPO4 solution. pKa is 7.21. А. 5.5 В. 6.5 O C. 4.5 O D. 7.5 30. Determine the ph of a 0.30 M NaH2PO4 and 0.20 M H3P04 solution. pka is 2.16. А. 1.3 В. 2.3 С. 3.3 D. 4.3

29. Determine the ph of a 0.50 M NaH2PO4 and 0.10 M Na2HPO4 solution. pKa is 7.21. А. 5.5 В. 6.5 O C. 4.5 O D. 7.5 30. Determine the ph of a 0.30 M NaH2PO4 and 0.20 M H3P04 solution. pka is 2.16. А. 1.3 В. 2.3 С. 3.3 D. 4.3

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

15. What is the pH of 0.630 M CH3NH2Cl solution? (kb of CH3NH2 = 3.45 x 10-5) A. 9.13 B. 4.10 C. 5.75 D. 4.87 E. 5.90
3. In the reaction below, H2O is a(n): H2SO; +H20 → H;0*+HSO; b. acid a. Base Sue conjugate acid d. conjugate base 4. What is the pH of a 1.53 x 10-6 M solution of HCl? c. 6.99 a. 5.82 b. 8.18 d. 4.15 5. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is 1.8x10- Calculate its pH value. a. 0.698 b. 2.72 с. 11.28 d. none of the answer are correct 6. Naz CO; forms alkaline solution when dissolved in water. Why? a. Because water hydrolysis produces hydroxide b. CO32- ions reacts with H from water to produce HCO; c. Na, CO; dissociates completely to produce CO;2- ions d. CO;?- ions reacts with water to produce carbonic acid The buffar celutien
1. a. Tris (C4H6(OH)3NH2) has a Ka of 7.94 x 10−9. Calculate the Kbfor this compound. b. If a chemist was to make 50.0 mL 0.20 M solution of Tris, what would the pH be after an addition of 10.0 mL of 0.10 M HCl?
17. Find the pH of 0.3500 M HNO₂(ag) solution @ 25 °C. K, for HNO₂ = 4.6 x 10-4 HNO₂ + H₂O NO₂ + H₂O+ A. 4.79 B. 3.79 C. 6.55 D. 8.72 18. What is the percent ionization of a 3.34 M solution of nicotinic acid, HC6H4NO₂? (K₂ = 1.4 x 10-5 @ 25 °C) HC6H4NO₂ + H₂O C6H4NO₂ + H₂O+ A. 4.68% B. 6.84 % C. 0.2% D. 48.8%
1. What is the pH of an aqueous solution if the [OH -] = 1.35 x 10 -5 M? A. 8.87 B. 5.13 C. 4.87 D. 9.13 E. 1.26 2. How many grams of water are needed to prepare 100.0 g of a 10.0% by mass cupric sulfate solution? A. 100g B. 90g C. 10g D. 1000g E. 75g 3. If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the solution would be considered: A) saturated. B) dilute. C) unsaturated. D) supersaturated. E) none of the above 4. Which of the following illustrates the like dissolves like rule for a solid in a liquid solvent? an ionic compound is soluble in a polar solvent a polar compound is soluble in a polar solvent a nonpolar compound is soluble in a nonpolar solvent all of the above none of the above 5. A hypertonic glucose solution: A. Causes cell hemolysis B. Has the same osmotic…
A 0.280 M solution of hydroxylammonium has a pH of 3.30. What is the Ką of hydroxylammonium? O a. 9.0 x 10-7 O b. 6.05 c. 5.0 x 10-4 d. 1.8 x 10-3 e. 2.5 x 10-7 What is the pH of a 0.797 M solution of hydroxylamine, a weak base with a Kp of 9.1 x 10- 9? O a. 9.93 O b. 4.07 O c. 5.96 O d. 8.04 O e. 13.90 A buffer solution containing 0.27 M benzoic acid and 0.33 M of the conjugate base, benzoate, was prepared. The pka of benzoic acid is 4.20. What is the pH of this buffer solution? a. 4.29 b. 4.11 c. 9.89 O d. 2.38 Ое. 4.20 A solution was found to have a pOH of 3.82 at 25 °C. What is the pH of this solution? a. 10.18 O b. -3.82 О с. -17.82 O d. 3.82 е. -10.18
245. What is the final pH of a 1.0 L solution containing 0.25 M HF, 0.75 M NaF, and 0.10 moles of KOH? Ka of HF is 7.1 x 10-4 a. 2.8 b. 3.9 c. 3.4 d. 2.3 e. 4.3
9. Calculate the pH of a 0.10 M aqueous solution of acetic acid. (CH3COOH, 60.02 g/mol, K₂= 1.8 x 105) a. 8.6 b. 2.9 c 7.0 d. 3.7 e. 4.2
5. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is 1.8x10-5 . Calculate its pH value. a. 0.698 b. 2.72 c. 11.28 d. none of the answer are correct 6. Naz CO3 forms alkaline solution when dissolved in water. Why? a. Because water hydrolysis produces hydroxide b. CO32- ions reacts with Ht from water to produce HCO3 c. Naz CO3 dissociates completely to produce CO;2- ions d. CO32- ions reacts with water to produce carbonic acid 7. The buffer solution maintains pH by some events except a. The addition of a little acid b. The addition of a little base c. Addition of water d. The addition of excess acid 8. Which of the following is TRUE about buffer solution? a. pH of buffer solution will never change despite addition of small amount of base or acid b. Buffer can be made by mixing strong acid and salt ot its conjugate base or by mixing strong base with salt of its conjugate acid
5. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is 1.8x10- Calculate its pH value. a. 0.698 b. 2.72 c. 11.28 d. none of the answer are correct 6. Naz CO; forms alkaline solution when dissolved in water. Why? a. Because water hydrolysis produces hydroxide b. CO32- ions reacts with H from water to produce HCO;- c. Naz CO; dissociates completely to produce CO;2-ions d. CO3?- ions reacts with water to produce carbonic acid The buffar celutien nintoing nH
The pain killer morphine is a weak base when added to water. Morphine has a pKb of 5.796 and dissociates similar to ammonia in aqueous solutions. What is the pH of a 5.00 x 10 -3 M solution of morphine? a. 11.3 b. 9.95 c. 8.23 d. none of these e. 10.2
6. What is the pH of a solution containing 0.550 M HOAc and 0.460 M LiOAc?(ka of HOAc = 1.80 x 10-5) A. 4.95 B. 2.50 C. 4.67 D. 6.40 E. 8.72