Look at the titration curve below and determine what acid from the list could be the acid beingtitrated with NaOH. The black colored circle represents the equivalence point.O(A) HCNO Ka = 3.5 × 10-4 (B) H2C2O4 Ka = 5.9 × 10-2(C) HCHO₂ Ka = 1.8 × 10-4 (D) HC (E) HN3 Ka = 1.9 × 10-5pH7.03.4602550Submitvolume NaOH added

Step 1: Determine the volume at the equivalence point. From the given titration curve the volume at…

Answered: Look at the titration curve below and…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 52SSC

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8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Assume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl. (a) What is the pH of the NH3 solution before the titration begins? (b) What is the pH of the equivalence point? (c) What is the pH at the midpoint of the titration? (d) Which indicator would you suggest to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 11.0, 15.0, 20.0, 22.0, and 25.0 mL of the acid. Combine this information with that from (a) through (c) and plot the titration curve.
The titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH. The reaction can be represented as: CH3 CO2 H + OH− ⟶ CH3 CO2− + H2 O(a) What is the initial pH before any amount of the NaOH solution has been added? Ka = 1.8 × 10−5 for CH3CO2H. (b) Find the pH after 25.00 mL of the NaOH solution have been added.(c) Find the pH after 12.50 mL of the NaOH solution has been added.(d) Find the pH after 37.50 mL of the NaOH solution has been added.
In the titration of 60.0 mL of 1.0 M methylamine, CH3NH₂ (K₁ = 4.4 x 10-4), with 0.50 M HCI, calculate the pH under the following conditions. (a) after 0.00 mL of 0.50 M HCI has been added 4.0 (b) after 20.0 mL of 0.50 M HCI has been added 4.0✔ (c) after 60.0 mL of 0.50 M HCI has been added 4.0✔ (d) at the stoichiometric point 4.0✔ (e) after 200.00 mL of 0.50 M HCI has been added 4.0
a) What will be the H+ concentration in a 1.0 M HCN solution? (HCN is a weak acid: Ka = 4.0x10-1) b) Methylamine is a weak base. Calculate the pH of a 0.2 M aqueous solution of methylamine. The Kb = 3.6 x 10-4 c) In a titration, 15.0 mL of 0.100 M phosphoric acid H3PO4 neutralises 30.0 mL of a solution of calcium hydroxide Ca(OH)2. What is the M of the solution of calcium hydroxide?
Calculate the pH of the following buffer solutions:(A-) 10 mL 0.1 H3po4 + 25 mL 0.1 NaOH (B-) 10 mL 0.1 H3PO4 + 25 mL 0.1 Na3 PO4 (C- )A buffer solution pH=5.00 contains 0.01 M CH3 COOH.Calculate the concentration of sodium acetate it contains.(D- )What weight of NH4CI should be added to 1 L of 0.1 MNH3 solution to get pH=9.00?
You need to make 1.0 L of a buffer solution having pH = 4.30 from CH3COOH and NaCH3COO. What concentrations of CH3COOH and NaCH3CO0 will you have to prepare? [Hint: Various concentrations are available. You need to explain your answers with reasonable rationale.] Ka for CH3COOH= 1.8 × 10–5
Calculate the pH of a buffer system containing 3.0 M NH3 and 2.0 M NH4Cl. (K, of NH4, the acid in this system, is 5.6 x 10-10.) Enter your answer in the provided box. PH
Calculate the pH of a buffer system containing 1.5 M NH3 and 1.5 M NHẠCI. (K, of NH, the acid in this system, is 5.6 x 1010.) Enter your answer in the provided box. pH =
3. A 20.0 mL sample of 0.200 M cyanic acid (HOCN, Ka-3.3 x 104) is titrated with 0.400 M NaOH. Calculate the pH and % dissociation of the cyanic acid solution before any NaOH solution has been added. (a) (b) Calculate the pH of the solution after 3.00 mL of NaOH solution has been added. Calculate the pH of the solution at the half equivalence point. (c) (d) Calculate the pH of the solution at the equivalence point. and I 11
TUTOR Analysis of a Weak Acid-Strong Base Titration Curve Determine the pH during the titration of 63.3 mL of 0.465 M formic acid (K₂ = 1.8×10) by 0.465 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 95.0 mL of KOH

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