Problem 17.40 - Copy Assume that 32.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HX. Part A How many moles of HX have been added at the equivalence point? Express your answer using two significant figures. IVE ΑΣΦ n = Submit Part B Request Answer What is the predominant form of B at the equivalence point? BH (aq) BH+ (aq) BX (aq) BX+ (aq) Submit ? Request Answer mol

Problem 17.40 - Copy Assume that 32.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HX. Part A How many moles of HX have been added at the equivalence point? Express your answer using two significant figures. IVE ΑΣΦ n = Submit Part B Request Answer What is the predominant form of B at the equivalence point? BH (aq) BH+ (aq) BX (aq) BX+ (aq) Submit ? Request Answer mol

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

#19.16
Question 1 of 5 What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 10 4) and 0.200 mol of NaF to which 0.140 mol-of NaOH were added? 2.879 1 6. 8. 9. +/- 0. O Type here to search 68 3. 2. LO 4.
please explain then give answer
One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used? please explain than solve
2. No need to explain too much
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )
Given: IO31- + 6 H1+ + 6 S2O32- --> 3 S4O62- + I1- + 3 H2O If 13.98 mL of 0.184 M S2O32- Are required to titrate 5.00 mL of IO31- solution, what is the M of the IO31- ion in the original solution.
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74? Question 2 options: NH3 / NH4Cl (Ka = 5.6 × 10–10) NaNO2 / HNO2 (Ka = 4.5 × 10–4) CH3COONa / CH3COOH (Ka = 1.8 × 10–5) NaCl / HCl NaOCl / HOCl (Ka = 3.2 × 10–8)
A triprotic acid is titrated with KOH. What species are NOT in solution to any large extent between the 1st and 2nd equivalence points? Select all that apply. O H3A O HA? O A³- K+ O OH H2A
What is the highest pH that could be used as an effective buffer with B (a generic base) with Kp = (6.46x10^-10) and its chloride salt, HBCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
How many grams of dry NH4Cl need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.56? Kb for ammonia is 1.8×10−5 . Express your answer with the appropriate units. (Gpt/ai wrong answer not allowed)
What is the resulting molarity of LIOH after dilution (but BEFORE any possible chemical reaction) if (2.28x10^1) mL of (9.020x10^-1) M LİOH are mixed with (5.740x10^1) mL of (3.040x10^-1) M HCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.