**Problem Statement:**A certain weak base has a \( K_b \) of \( 8.00 \times 10^{-7} \). What concentration of this base will produce a pH of 10.31?**Solution Attempt:**An input box is provided with the label "concentration:", and the value entered is 0.003215.Below the input box, a message indicates "Incorrect".**Explanation:**To solve this problem, use the relationship between the base dissociation constant (\( K_b \)), the concentration of the base, and the pH. Given the pH, calculate the pOH and use this to determine the concentration of hydroxide ions (\( OH^- \)). Using these values, the concentration of the weak base needed to achieve the given pH can be calculated.The attempted concentration of 0.003215 returned an incorrect result, indicating a miscalculation. Adjustments to calculations or a re-evaluation of the approach may be needed.

Answered: A certain weak base has a Kp of 8.00 x…

A certain weak base has a Kp of 8.00 x 1'. What concentration of this base will produce a pH of 10.31? concentration: 0.003215 Incorrect

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

Related questions

Q: 3) Calculate the concentration (in M) of hydronium ions in a solution at 25.0 °C with a pOH of 3.58.…

A: Given:pOH of the solution = 3.58We have to determine the concentration (in M) of hydronium ions.

Q: Starting with 0.1 mol L−1 HNO2(aq), which one of the following operations would cause the pH of the…

Q: A 31.7 mL sample of a 0.399 M aqueous acetic acid solution is titrated with a 0.244 M aqueous sodium…

A: Given, Volume of 0.399 (M) acetic acid solution =…

Q: Determine the pH of a 0.62 M NH4NO3 solution at 25°C. The Kp for NH3 is 1.8 x 10-5. Express your…

Q: Which of the following aqueous solutions are good buffer systems? | 0.35 M ammonia + 0.30 M sodium…

A: Buffer solutions are the solutions containing a mixture of weak acid and its conjugate base or a…

Q: 6.) A 25.00 mL sample of HCL is titrated with 0.1001 M NaOH. 49.90 mL of base is required to reach…

Q: A solution is prepared that is initially 0.12M in hydrofluoric acid (HF) and 0.061 M in sodium…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all…

A: It refers to the acid dissociation constant having the significance of that fact that how much or…

Q: In an experiment, 1.000 mol H2 and 1.000 mol l2 are mixed in a 1.00-L container, and the reaction…

A: Equilibrium constant can be defined as number that represents the relationship between the amounts…

Q: . The concentration of an unknown weak acid solution is 0.20M, and the solution has a pH of 3.89.…

A: Since you have posted multiple questions, we are entitled to answer the first only. Given: Initial…

Q: A student prepares a solution by dissolving 4.17 g of solid KOH in enough water to make 200.0 mL of…

A: Given that, Molarity of KOH solution=0.372M 30.00 mL of this sample was taken and added into 500mL…

Q: When a 21.0 mL sample of a 0.342 M aqueous hydrocyanic acid solution is titrated with a 0.495 M…

Q: 6

A: When NaOH is added in the Solution then NaOH react with CH3COOH acid to form more salt, OH- ion…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: Reaction of solubility of M(OH)2 in water M(OH)2 (aq) →M2+(aq) + 2 O-H (aq)pH of solution 10.36pH +…

Q: When a 27.2 mL sample of a 0.349 M aqueous hydrocyanic acid solution is titrated with a 0.424 M…

Q: Which of the following aqueous solutions are good buffer systems? 0.26 M ammonia + 0.37 M calcium…

Q: When a 19.4 mL sample of a 0.395 M aqueous acetic acid solution is titrated with a 0.345 M aqueous…

A: Given, Volume of acetic acid = 19.4 mL Concentration of acetic acid = 0.395 M Volume of KOH = 33.3…

Q: When a 27.7 mL sample of a 0.426 M aqueous hydrocyanic acid solution is titrated with a 0.500 M…

A: we need to calculate the pH of solution

Q: When a 27.4 mL sample of a 0.492 M aqueous hydrofluoric acid solution is titrated with a 0.412 M…

A: When we add NaOH solution to HF solution first base will neutralize acid present in solution, excess…

Q: Solid barium nitrite is slowly added to 75.0 mL of a ammonium phosphate solution until the…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: When a 19.3 mL sample of a 0.316 M aqueous acetic acid solution is titrated with a 0.448 M aqueous…

Q: You are running a titration. You have placed 40.0 mL of 0.200 M chlorous acid, HCIO2, in a flask and…

A: mmoles of HClO2 = 40 x 0.2 = 8 mmoles mmoles of KOH = 80 x 0.1 = 8 mmoles KOH + HClO2 ----->…

Q: 6. Calculate the pH of the solution that results when0.093 g of Mg(OH)2 is mixed with 75.0 mL of…

Q: 1) What is the pH at the equivalence point in the titration of a 29.1 mL sample of a 0.450 M aqueous…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: A 46.9 mL sample of a 0.347 M aqueous acetic acid solution is titrated with a 0.494 M aqueous…

Q: 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium,…

A: Given: Initial moles of HA = 0.030 moles Volume of container = 2.0 L Equilibrium concentration of HA…

Q: When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueous…

Q: Which of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M…

A: A good buffercalled as relatively equal concentrations of a weak acid and its conjugate base.

Q: Which of the following aqueous solutions are good buffer systems? O0.13 M hypochlorous acid + 0.12 M…

A: Option D is the correct choice among the given buffers. A buffer solution is one which can resist…

Q: A Chemistry student is asked to predict the pH of a potassium hydroxide solution when 1.82 g of…

A: KOH is a strong electrolyte. So it will completely dissociate when it will be dissolved in water.…

Q: When a 29.6 mL sample of a 0.356 M aqueous hydrocyanic acid solution is titrated with a 0.366 M…

A: The volume of the aqueous hydrocyanic acid = The concentration of the aqueous hydrocyanic acid = The…

Q: please step by step solution.

A: Part 1. Given:…

Q: A sample of 25.0 mL of buffer solution contains 0.100 M fluoride ions and 0.126 M hydrofluoric acid.…

A: 25.0 mL of buffer solution0.100 M fluoride ions0.126 M HF4.93 mL of 0.0100 M HCl is added to the…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

100%

**Problem Statement:**

A certain weak base has a \( K_b \) of \( 8.00 \times 10^{-7} \). What concentration of this base will produce a pH of 10.31?

**Solution Attempt:**

An input box is provided with the label "concentration:", and the value entered is 0.003215.

Below the input box, a message indicates "Incorrect".

**Explanation:**

To solve this problem, use the relationship between the base dissociation constant (\( K_b \)), the concentration of the base, and the pH. Given the pH, calculate the pOH and use this to determine the concentration of hydroxide ions (\( OH^- \)). Using these values, the concentration of the weak base needed to achieve the given pH can be calculated.

The attempted concentration of 0.003215 returned an incorrect result, indicating a miscalculation. Adjustments to calculations or a re-evaluation of the approach may be needed.

Expert Solution

Step 1

The given pH is 10.31

Kb = 8.00 x 10^-7

pOH = 14-10.31 = 3.69

[OH-] = 10^-3.69 = 0.000204173

Step by step

Solved in 2 steps

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Help please
Fill out the tables and find pH
Which of the following additions will result in a decrease in the pH of the solution? Adding ammonium nitrate to an ammonia solution. Adding potassium chloride to a hydrochloric acid solution. Adding sodium formate to a formic acid solution.
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
A certain weak base has a Kp of 8.50 x 10-'. What concentration of this base will produce a pH of 10.24? concentration:
Calculate the pH of a 0.300 M NH4Cl solution. Kp for NH3 is 1.8 x 10-5.
When a 15.2 mL sample of a 0.316 M aqueous nitrous acid solution is titrated with a 0.337 M aqueous sodium hydroxide solution, what is the pH after 21.4 mL of sodium hydroxide have been added?pH =
When a 22.9 mL sample of a 0.351 M aqueous acetic acid solution is titrated with a 0.445 M aqueous potassium hydroxide solution, what is the pH after 27.1 mL of potassium hydroxide have been added? pH =
1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
Please answer all the three the questions as soon as possible Thank you so much! 3. Solid silver nitrite is slowly added to 125 mL of a sodium cyanide solution until the concentration of silver ion is 0.0523 M. The maximum amount of cyanide remaining in solution is M.
When a 15.4 mL sample of a 0.479 M aqueous hydrocyanic acid solution is titrated with a 0.457 M aqueous sodium hydroxide solution, what is the pH after 24.2 mL of sodium hydroxide have been added?pH =