### Problem StatementDr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL, calculate the pH of the new solution. Assume that no dissociation takes place until the new solution is made. The dissociation constant, $ K_a $, for nitrous acid is $ 4.6 \times 10^{-4} $.### Chemical Reaction\[ \text{HNO}_2(aq) + \text{H}_2\text{O}(l) \rightarrow \text{H}_3\text{O}^+(aq) + \text{NO}_2^-(aq) \]### Explanation1. **Dilution Calculation:** - Initial concentration ($ C_i $) = 0.4 M - Initial volume ($ V_i $) = 3 mL - Final volume ($ V_f $) = 100 mL Use the dilution formula: \[ C_f = \frac{C_i \times V_i}{V_f} \] Calculate the new concentration ($ C_f $) after dilution.2. **pH Calculation:** - Use the dissociation constant ($ K_a $) to find the concentration of $ \text{H}_3\text{O}^+ $. - Calculate the pH using: \[ \text{pH} = -\log [\text{H}_3\text{O}^+] \]The task involves using chemical equilibrium concepts to find the pH of the solution after dilution.

we have to calculate the pH of solution

2. Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL calculate the pH of the new solution. (assume that no dissociation takes place until the new solution is made.) Ka = 4.6´ 10-4 HNO₂(aq) + H₂O(1) NO₂ (aq) H,O*(aq) +

2. Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL calculate the pH of the new solution. (assume that no dissociation takes place until the new solution is made.) Ka = 4.6´ 10-4 HNO₂(aq) + H₂O(1) NO₂ (aq) H,O*(aq) +

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 110CWP

See similar textbooks

Related questions

Q: Write the equilibrium constant expression for this reaction: H;PO,(aq) - 3 H (aq)+PO (aq)

Q: Consider the following data on some weak acids and weak bases: acid base K, K, name formula name…

A: In this question we will be dealing with salts of strong acid + weak base and salts of weak acid +…

Q: Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine…

Q: Calculate the pH of a solution by dissolving 1.90 g of sodium acetate, CH3COONa, in 71.0 mL of 0.15…

A: Given,the mass of sodium acetate ( CH3COONa ) = 1.90 gmolarity of acetic acid ( CH3COOH ) = 0.15…

Q: Which of the following reactions accurately shows how Fe" acts as an acid in water? A) Fe(OH), (s) =…

A: Fe3+ is a Lewis acid, which can be defined as the chemical species containing an empty orbital and…

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: Solution X 100 mL of 0.10 M NaOH(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Y 100 mL of…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: The concept used over here is-Weak acid HA does not dissociate entirely, so it remains in the water.…

Q: Calculate the pH and the pOH of these solutions:

Q: Acidity of a solution is determined by the concentration H of hydrogen ions in the solution…

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

### Problem Statement

Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL, calculate the pH of the new solution. Assume that no dissociation takes place until the new solution is made. The dissociation constant, $ K_a $, for nitrous acid is $ 4.6 \times 10^{-4} $.

### Chemical Reaction

\[ \text{HNO}_2(aq) + \text{H}_2\text{O}(l) \rightarrow \text{H}_3\text{O}^+(aq) + \text{NO}_2^-(aq) \]

### Explanation

1. **Dilution Calculation:**
- Initial concentration ($ C_i $) = 0.4 M
- Initial volume ($ V_i $) = 3 mL
- Final volume ($ V_f $) = 100 mL

Use the dilution formula:

\[
C_f = \frac{C_i \times V_i}{V_f}
\]

Calculate the new concentration ($ C_f $) after dilution.

2. **pH Calculation:**
- Use the dissociation constant ($ K_a $) to find the concentration of $ \text{H}_3\text{O}^+ $.
- Calculate the pH using:

\[
\text{pH} = -\log [\text{H}_3\text{O}^+]
\]

The task involves using chemical equilibrium concepts to find the pH of the solution after dilution.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

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

Hello please help me with my homework fast.
4 F Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. R V Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. $2 CH,COO species Explanation NH3 CH₂CH(OH)COO CH₂CH(OH)COOH 5 % NH CH₂COOH H₂O G T H₂O* B Check 20 6 relative pH of 0.1 M aqueous solution Y H (Choose one) ▼ (Choose one) ▼ 8 (highest) (Choose one) ▼ 6 (Choose one) ▼ N 1 (lowest) MacBook Pro 7 U J * 8 M 1 X K ( 9 Ś O ) O L © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…
When is it safe to assume that the change from initial concentration (+/- x) is small enough to be negligible/ignore when doing equilibrium calculations for weak acids and bases? Be specific!
Calculate the pH of a weak base which dissociates as BOH ⇌ B+ + OH- ( like NH3 (g) + H2O(l) → NH4OH(aq) , where in water NH4OH ⇌ NH4+ + OH- ) knowing that the initial concentration of the base is 1.04 M, and the base dissociation constant, Kb , is 3.79e-10. pH ← please insert your value
Ascorbic acid (H, C,H,0,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and K„2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. 2.49 pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O,] = 0.131 M [HC,H,0G] = 3.22 x10-3 M 7.18 x10 -8 [C,H,O; = M Incorrect
•x H₂O 7 8 Submit 个 Tap here or pull up for additional resources 9 (aq) Br H₂O OH- O
please correct name for #9
At equilibrium, the [H+] in a 2.50M solution of a weak acid, HA, is 4.07x10-3M. a) Write an equation for dissociation for this unknown weak acid, HA. b) Write the Ka expression for this unknown acid. c) What are the equilibrium concentrations of all species for this unknown acid? d) What is the pH, pOH and % ionization of this weak acid?
-10 The acid dissociation constant K of boric acid (H,BO, is 5.8 x 10 . Calculate the pH of a 6.0 M solution of boric acid. Round your answer to 1 decimal place. PH pH = ?
Determine the Kb for a base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > The pH for a 0.0160 M solution of CH:CH.NH: is 8.600. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. CH:CsH&NH:(aq)+ H:O(1) OH-(aq) +CH:CeH&NH;*(aq) Initial (M) |Change (M) Equilibrium (M) 5 RESET 0.0160 8.60 -8.60 0.93 -0.93 2.50 x 109 -2.50 x 109 3.98 x 10 -3.98 х 10° 5.4 -5.4
Ascorbic acid (H,C,H,O,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and Ka2 = 1.60 x 10-12. Determine the pH of a 0.118 M solution of ascorbic acid. 4.09 pH Incorrect Determine the equilibrium concentrations of all species in the solution. [H,C,H,O.] M %3D Incorrect [HC,H,0;] = M Incorrect (C,H,0;-] =| M Incorrect
Ethylamine has Kb=4.3x10^-4. Calculate the pH if the initial concentration is 0.15 M. Write the dissociation reaction