C. What is the pH if 30.0 mL of 0.20M NaH2PO4 was mixed with 35.0 mL of 0.30M NazHPO4? The pKa values of phosphate are 2.14, 7.20 and 12.40. D. What is the pH if 28.0 mL of 0.570M phosphoric acid is added to 110.0 mL of 0.4800M monosodium dihydrogen phosphate? The pKa values of phosphate are 2.14, 7.20 and 12.40.

C. What is the pH if 30.0 mL of 0.20M NaH2PO4 was mixed with 35.0 mL of 0.30M NazHPO4? The pKa values of phosphate are 2.14, 7.20 and 12.40. D. What is the pH if 28.0 mL of 0.570M phosphoric acid is added to 110.0 mL of 0.4800M monosodium dihydrogen phosphate? The pKa values of phosphate are 2.14, 7.20 and 12.40.

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

Calculate the pH values and draw the titration curve for the titration of 500 mL of 0.010 M acetic acid (pKa 4.76) with 0.010 M KOH. Part A Calculate the pH of the solution after 0 mL of the titrant have been added. Express your answer to two decimal places. VE ΑΣΦ pH = Submit Part B pH = Request Answer Calculate the pH of the solution after 250 mL of the titrant have been added. Express your answer to two decimal places. VE ΑΣΦ Submit Request Answer Part C = ? ? Calculate the pH of the solution after 450 mL of the titrant have been added. Express your answer to two decimal places.
Which of the following is true about the titration curves of solutions of weak acids? A. The pH for optimal buffering power of a weak acid is 7.00. B. You can calculate the pKa of an acid, given the pH and the molar ratio of the acid and its conjugate base. C. The pKa of a weak acid is the pH at which the acid is completely dissociated. D. At a pH below the pKa of a weak acid, its conjugate base will predominate.
Which of the following is the best buffer at neutral pH (pH 7.0)? a) Acetic acid, pKa = 4.76 b) Carbonic acid, pKa1 = 3.6; pKa2 = 10.3 c) Water, pKa = 14 d) Phosphoric acid, pKa1 = 2.15; pKa2 = 7.2; pKa3 = 12.35
85 ml of 0.5M sodium acetate is combined with 15 ml of 0.5 M acetic acid. What is the pH of the solution?(Hint: the pKa of acetic acid is 4.76)
A titration of 200.0 mL of 2.55 MH 2A was done with 1.00 M NaOH. For the diprotic acid H 2A, Ka1 =2.5 x 10-5, Ka2=3.1 x 109. Calculate the pH before any 1.00 M NaOH has been added. Oa. 11.83 Ob.8.68 O c. 9.66 Od.2.17 Oe. 4.20
ETUSTUOto 3JAT 0 520 | CHAPTER 14 Acids and Bases 49. A 25.00-mL sample of an H₂SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the un- known H₂SO4 solution? 52 51. What volume in milliliters of a 0.121 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 10.0-mL sample of 0.102 M sulfuric acid? NG AND WEAK ACIDS AND BASES assify each acid as strong or weak. HCI HF Br 2SO3 50. 52 5
55. Human blood is buffered by carbonic acid and bicarbonate ions. Alkalosis is a condition caused by excess production of bicar- bonate in the blood. A patient's blood plasma has a pH = 7.6 (pKa for H2CO3 at body temperature is 6.1). MISSED THIS? Read Section 18.2; Watch KCV 18.2B, IWE 18.2, 18.3 [HCO3] [H2CO3] a. What is the ratio of in the patient's blood? b. The doctor gives the patient 0.45 g of HCl intravenously to neutralize alkalosis. After treatment, the patient's blood is 0.0156 M in HCO3¯ and 0.0012 M in H2CO3. If the volume of blood in the patient's body is 5.3 L, what is its new pH?
Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH of 7.60. She adds 10.0 mL of 1.0 M HCl, which changes the pH to 3.00. The pKa value of one of the groups is pK₁ = 3.70 and it is known that pK2 is between 7 and 10. What is the exact value of pK₂? pK₂ =
What is the pH of the solution containing 0.25 M NH3 and 0.09 M NH4C1? ; pka = 9.25 (Show your solution:
You have a solution of nitrous acid (HNO2). What effect will addition of sodium nitrite (NaNO2) have on the pH of the solution? Ka for nitrous acid = 4.5 ´ 10-4
A 15.00 mL sample of 0.355 M H3PO4 (Ka,1 7.52 × 10-3, Ka,2 6.23 × 10-8, Ka3 2.1 × 10-13) is titrated with 0.485 M NaOH. a. What is the pH of the solution after 1.50 mL of NaOH has been added? Hint: The first equivalence point has not been reached. b. What volume of NaOH is needed to reach the third equivalence point?