Explanation Given that, the buffer contains 0.040 M N a C H 3 C O 2 ( a q ) and 0.080 M C H 3 C O O H ( a q ) . The addition of a base will react with the weak acid and thus decreases the concentration of weak acid and increases the concentration of conjugate base. The proton transfer equilibrium is given below. C H 3 C O O H ( a q ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + C H 3 C O 2 − ( a q ) K a = [ H 3 O + ] [ C H 3 C O 2 − ] [ C H 3 C O O H ] = 1.8 × 10 − 5 The reaction of added base with some of C H 3 C O O H is given below. C H 3 C O O H ( a q ) + O H − ( a q ) → C H 3 C O 2 − ( a q ) + H 2 O ( l ) The initial number of moles of acid can be calculated as shown below. n ( C H 3 C O O H ) i n i t i a l = 0.300 L × 0.080 m o l . L − 1 = 0.024 m o l The molar ratio of acid and added base in the above equation is 1 : 1. The number of reacted moles of acid after addition of 0.0200 m o l o f N a O H can be calculated as given below. n ( C H 3 C O O H ) r e a c t s = 0.0200 m o l O H − × 1 m o l C H 3 C O O H 1 m o l O H − = 0.0200 m o l C H 3 C O O H Now, the remaining amount of acid can be estimated. n f i n a l = n i n i t i a l − n r e a c t s = 0

7th Edition

ISBN: 9781319420994

Author: ATKINS

Publisher: MAC HIGHER

See similar textbooks

Question

Chapter 6, Problem 6G.2AST

Interpretation Introduction

Interpretation:

The pH of the resulting solution and the change in pH has to be calculated.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 6, Problem 6G.1BST

Chapter 6, Problem 6G.2BST

Students have asked these similar questions

A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10–4 Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer.

The solubility of TICI (thallium(I) chloride), an intermediate formed when thallium is being isolated from ores, is 3.12 grams per liter at 20 °C. What is its solubility product?

Calculate the molar solubility of Mg(OH)2 in 1.00 M NH4Cl (aq).

Chapter 6 Solutions

CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM

Ch. 6 - Prob. 6A.1AST Ch. 6 - Prob. 6A.1BST Ch. 6 - Prob. 6A.2AST Ch. 6 - Prob. 6A.2BST Ch. 6 - Prob. 6A.3AST Ch. 6 - Prob. 6A.3BST Ch. 6 - Prob. 6A.1E Ch. 6 - Prob. 6A.2E Ch. 6 - Prob. 6A.3E Ch. 6 - Prob. 6A.4E

Knowledge Booster

The p H of the resulting solution and the change in p H has to be calculated.

Solution Summary: The author explains that the pH of the resulting solution and the change in pH has to be calculated.

Interpretation:

The pH of the resulting solution and the change in pH has to be calculated.

Want to see the full answer?

Chapter 6 Solutions

The p H of the resulting solution and the change in p H has to be calculated.

Solution Summary: The author explains that the pH of the resulting solution and the change in pH has to be calculated.

Interpretation: The pH of the resulting solution and the change in pH has to be calculated.

Want to see the full answer?

Chapter 6 Solutions

Interpretation:

The pH of the resulting solution and the change in pH has to be calculated.