A chemistry graduate student is given 300. mL of a 0.50M dimethylamine ((CH3)2NH) solution. Dimethylamine is a weak base with K = 5.4 × 10(CH3)2NH2Br should the student dissolve in the (CH3)2NH solution to turn it into a buffer with pH = 10.617You may assume that the volume of the solution doesn't change when the (CH3)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round itto 2 significant digits.☐x10

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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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-4 What A chemistry graduate student is given 100. mL of a 1.10 M trimethylamine ((CH,) N) solution. Trimethylamine is a weak base with K, = 7.4 x 10 mass of (CH, NHB1 should the student dissolve in the (CH, N solution to turn it into a buffer with pH = 10.56? You may assume that the volume of the solution doesn't change when the (CH, NHB is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
How many grams of sodium formate, HCOONa, are required to mix with 1.50 Liters of 0.500 M formic acid, HCOOH, in order to prepare a buffer solution with a pH that equals 4.00? pKa(HCOOH) = 3.74 and MM(HCOONa) = 52.01 g/mol
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10
A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH solution. Dimethylamine is a weak base with K,=5.4 × 10 . What mass of (CH,), NH, Cl should the student dissolve in the (CH,) NH solution to turn it into a buffer with pH =10.80? You may assume that the volume of the solution doesn't change when the (CH, NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 10
A chemistry graduate student is given 500.mL of a 0.80M chloroacetic acid (HCH2ClCO2) solution. Chloroacetic acid is a weak acid with Ka = 1.3x10^−3. What mass of NaCH2ClCO2 should the student dissolve in the HCH2ClCO2 solution to turn it into a buffer with pH = 3.08 ?You may assume that the volume of the solution doesn't change when the NaCH2ClCO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO
A buffer consists of 0.12 M NaH2PO4 and 0.33 M Na2HPO4. Phosphoric acid is a triprotic acid (Ka1 = 7.2 × 10−3, Ka2 = 6.3 × 10−8, Ka3 = 4.2 × 10−13) Which Ka value is most important to this buffer? What is the buffer pH? .
-5 %3D A chemistry graduate student is given 450. mL of a 0.30 M acetic acid (HCH,CO,) solution. Acetic acid is a weak acid with K = 1.8 × 10 . What mass of a NaCH,CO, should the student dissolve in the HCH,CO, solution to turn it into a buffer with pH =4.29? 2
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How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 2.80? (Ka for HF is 6.8 × 10⁻⁴)
Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl (Correct answer) 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH please explain. thanks!

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