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Acid - Base Worksheet Name 1. A chemistry student titrated several solutions of unknown concentrations with...
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...
Acid/Base titrations 10. 25.0 mL of 0.100 M H2A (a weak diprotic acid) is titrated with...
Acid/Base titrations 10. 25.0 mL of 0.100 M H2A (a weak diprotic acid) is titrated with 0.200 M NaOH. What is the pH of the solution when 0.00 mL, 10.0 mL, 12.5 mL, 20.0 mL, 25.0 mL, and 40.0 mL E.S RaWeMA 5.83 x 10 8) have been added? (Ka1= 2.46 x 10, Ka2 ANSWER: 0 mL = 2.315, 10.0 mL= 4.211 (or 4.213), 12.5 mL = 5.422, 20.0 mL 7.410, 25.0 mL = 9.966, 40.0 mL = 12.664 11....
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 15.0 mL of KOH. Exp...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 15.0 mL of KOH. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part C A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part D A 52.0-mL volume of 0.35 M CH3COOH...
Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following...
Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution Part A Calculate the concentration (in M) of the unknown HCl solution in the first case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 20.00 mL 27.44 mL 0.1191 M HCI Volume (mL) 20.00 mL 14.00 mL...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2?
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg = 1.8 x 10-5. b. 35.0 mL of 0.175 M NH3 is mixed with 15.0 mL of 0.10 M HCl. c. 50.0 mL of 0.275 M acetic acid is mixed with 100. mL of 0.100 M HCl. d. The equivalence point of a 50.0 mL solution of 0.120 M acetic acid titrated by 0.100 M NaOH.
Exercise 14.47 Review Part Four solutions of unknown HCl concentration are titrated with solutions of NaOH....
Exercise 14.47 Review Part Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the concentration (in M) of the unknown HCl solution in the third case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 24.00 mL 13.88 mL 0.1178 M Express your answer using four significant figures....
Four solutions of unknown NaOH concentration are titrated with solutions of HCl. The following table lists...
Four solutions of unknown NaOH concentration are titrated with solutions of HCl. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. NaOH Volume (mL) HCl Volume (mL) [HCl] (M) 7.00 mL 9.17 mL 0.2099 M 18.00 mL 10.84 mL 0.1111 M 15.00 mL 10.75 mL 0.0489 M 26.00 mL 35.18 mL 0.1421 M Part A: Calculate the concentration (in M)...
A student titrated 15.0 mL of acetic acid acid, HC2H302 ( Molar mass= 60 g/mol) solution...
A student titrated 15.0 mL of acetic acid acid, HC2H302 ( Molar mass= 60 g/mol) solution with 25.0 mL of a 0.100 M NaOH solution The Molarity(mol/L) of HC2H302 required for complete titration is? HC2H302 + NaOH - NaC2H302 + H20 A) 0.0250 M B) 0.250 M C) 2.5M D) 0.0167M E) 0.167 mol
Four solutions of unknown HCl concentration are titrated with solutions of NaOH.
Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Part BCalculate the concentration (in M) of the unknown HCl solution in the second case.
Acid/Base titrations 10. 25.0 mL of 0.100 M H2A (a weak diprotic acid) is titrated with 0.200 M NaOH. What is the pH of the solution when 0.00 mL, 10.0 mL, 12.5 mL, 20.0 mL, 25.0 mL, and 40.0 mL E.S RaWeMA 5.83 x 10 8) have been added? (Ka1= 2.46 x 10, Ka2 ANSWER: 0 mL = 2.315, 10.0 mL= 4.211 (or 4.213), 12.5 mL = 5.422, 20.0 mL 7.410, 25.0 mL = 9.966, 40.0 mL = 12.664 11....
Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution Part A Calculate the concentration (in M) of the unknown HCl solution in the first case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 20.00 mL 27.44 mL 0.1191 M HCI Volume (mL) 20.00 mL 14.00 mL...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2?
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg = 1.8 x 10-5. b. 35.0 mL of 0.175 M NH3 is mixed with 15.0 mL of 0.10 M HCl. c. 50.0 mL of 0.275 M acetic acid is mixed with 100. mL of 0.100 M HCl. d. The equivalence point of a 50.0 mL solution of 0.120 M acetic acid titrated by 0.100 M NaOH.
Exercise 14.47 Review Part Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the concentration (in M) of the unknown HCl solution in the third case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 24.00 mL 13.88 mL 0.1178 M Express your answer using four significant figures....
A student titrated 15.0 mL of acetic acid acid, HC2H302 ( Molar mass= 60 g/mol) solution with 25.0 mL of a 0.100 M NaOH solution The Molarity(mol/L) of HC2H302 required for complete titration is? HC2H302 + NaOH - NaC2H302 + H20 A) 0.0250 M B) 0.250 M C) 2.5M D) 0.0167M E) 0.167 mol
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