3. A 25.0-mL sample of concentrated sulfuric acid, H2SO4, is diluted to 1.00 L and a 25.0-mL sample of the dilute acid is further diluted to 100. mL. Then a 10.0-mL sample of the latest solution is titrated with 0.1075 M NaOH. If 20.8 mL of the NaOH solution is required to neutralize the very dilute H2SO4 solution, what is the concentration of H2SO4 in the original concentrated acid? (A) 4.47 M (B) 8.94 M (C) 17.9 M (D) 23.2 M

3. A 25.0-mL sample of concentrated sulfuric acid, H2SO4, is diluted to 1.00 L and a 25.0-mL sample of the dilute acid is further diluted to 100. mL. Then a 10.0-mL sample of the latest solution is titrated with 0.1075 M NaOH. If 20.8 mL of the NaOH solution is required to neutralize the very dilute H2SO4 solution, what is the concentration of H2SO4 in the original concentrated acid? (A) 4.47 M (B) 8.94 M (C) 17.9 M (D) 23.2 M

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

Suppose that 42.00 mL of 0.150 M NaOH is added to 0.360 g of a weak acid, H3A. The excess NaOH is then titrated with 23.40 mL of 0.120 M HCl. What is the molar mass of the acid? a) 103 g/mol b) 241 g/mol c) 190 g/mol d) 310 g/mol
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
6. Acid/base titration is a common method to determine the molarities of acids or bases, the molarity of certain salts can also be determined by titration. It took 22.34 mL of 0.5861 M HCl solution to neutralize 25.00 mL NaNO₂ solution. The acid- dissociation constant of HNO₂ is 4.511 × 10-¹. NaNO₂ + HCl → HNO₂ + NaCl Please answer the following questions. A What is pH of the NaNO₂ solution before titration? Hint, calculate the molarity of the NaNO₂ solution first. pH = Please provider your answer below. ( Check answer 7²² B. M HCl solution was added to the NaNO2 solution? pH = 00 0 Please provider your answer below. What is the pH when 12.78 mL of 0.5861 (0) Check answer C. What is the pH when 14.39 mL of 0.5861 M HCl solution was added to the NaNO₂ solution AFTER the equivalence point? pH = Please provider your answer below. 00 0 °C? pH= Please provider your answer below. Check answer What is the pH at equivalence point at 25 A → ← Check answer ← $ H $
17
Consider the neutralization reaction 2 HNO, (aq) + Ba(ОН), (аq) — 2 Н, О() + Ва(NO,), (aq) A 0.120 L sample of an unknown HNO, solution required 30.1 mL of 0.250 M Ba(OH), for complete neutralization. What is the concentration of the HNO3 solution? concentration: M
help
The titration of 25.0 mL of an unknown concentration HNO2 solution requires 83.6 mL of 0.12 M LIOH solution. What is the concentration of the HNO2 solution (in M)? O 0.20 M O 0.40 M 0.10 M O 0.36 M O 0.25 M
7. A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of titration.
For a 50.00 mL sample of a citrus beverage to reach the phenolphthalein endpoint, 17.62 mL of 0.04166 M NaOH is required. Determine the acidity of the sample in terms of grams of citric acid per 100 mL.
A CHM 122 student considers an ionic compound M,X, that contains the metal cation M2 and the anion X. 7. The student determines that the molar solubility of M,X, is 2.7 x 10mol/L. What is the Kan value for this compound? Type your answer in the space below using scientific notation. (example: 0.012 = 1.2*10^-2)