**Question 31 of 35**What is the pH of a buffer made from 0.200 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in 2.0 L of solution? *Note: The image also includes a number pad, which is typically used for entering numerical answers.*

Given, the number of moles of HCNO =0.200 molenumber of moles of NaCNO =0.410 molevolume of solution =2.0 LKa for HCNO =3.5×10-4we are asked to calculate the pH of the buffer solution.Therefore, the pH of the buffer solution would be, pH =3.77

Answered: What is the pH of a buffer made from…

Science

Chemistry

What is the pH of a buffer made from 0.200 mol of HCNO (Ka = 3.5 × 10-4) and 0.410 mol of NaCNO in 2.0 L of solution?

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: A buffer is created by dissolving 0.303 moles of lactic acid and 0.197 moles of sodium lactate in…

Q: What is the pH of a buffer prepared by mixing 20.0 g of ethylamine, CH3CH2NH2, and 20.0 g of…

A: Given -> Weight of CH3CH2NH2 = 20.0 gm Weight of CH3CH2NH3Cl = 20.0 gm Volume= 2.00 L

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 10¯1º)

A: The given data contains, pH = 10. Ka=4.9×10-10

Q: What is the pH of a buffer prepared by combining 0.36 moles of a weak acid, HA, with 0.69 moles of…

Q: A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this…

Q: what is the ph of a buffer made from 0.080 mol of HCNO (Ka=3.5x10^-4) and 0.410 mol of NaCNO in 2.0…

A: In this question, we will determine the pH value of buffer solution which is made from the weak acid…

Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ка 3 (Ka = 2.5 x 10°) and 0.080 mol of KBRO…

A: Given : Moles of HBrO = 0.350 mol. Moles of KBrO = 0.080 mol. Ka of HBrO = 2.5 X 10-9 And volume of…

Q: How many grams of sodium hydroxide are needed to be added to 534 mL of 0.450 M HA solution to…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

Q: Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

A: Ka for acid = 1.8 x 10-5 [CH3COOH] = 1.0 M [CH3COONa] = 1.2 M PH = ?

Q: What is the pH of a buffer prepared by mixing 20.0 g of ethylamine CH3CH2NH2, and 20.0 g of…

Q: 1. What is the pH of a solution that results from adding 400 mL of 0.40 M NaOH to 600 mL of 0.50 M…

A: Note: As per the guidelines solution of 1st question has been made. For the expert solution of other…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

Q: What is the pH of the buffer that occurs when 7.00 Mol of H2SO4 and 4.0 Mol of NaOH are diluted with…

A: A buffer solution generally consists of a weak acid and its salt. Buffer solution resists the change…

Q: Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate inmuscles during intense…

A: The objective of this question is to calculate the pH of a buffer solution prepared by mixing lactic…

Q: What is the pH of a buffer made from 0.130 mol of HCNO (Ka=3.5*10^-4) and 0.410 mol of NaCNO in 2.0…

A: pH of the solution = 3.96

Q: What is the pH of a buffer

A: Buffer is a solution of weak acid and base. the pH of buffer can not changes with addition or acid…

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.150 mol of KBrO in…

Q: Calculate the pH of a buffer solution that is 0.41 M in HOCl and 0.50 M in NaOCl. [Ka(HOCl) = 3.24 x…

Q: A bottle with 0.5 L of ammonia (NH3) solution that is 13.2% by mass has a density = 0.9430 g/mL. How…

A: Given, Volume of ammonia solution =0.5L Density of ammonia solution = 0.9430g/mL Mass % of ammonia…

Q: What is the pH of a buffer made from 0.140 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 x 10-9) and 0.090 mol of KBrO in…

A: pKa = -log Ka = -log (2.5 x 10-9) = 9 -log2.5 = 9-0.40 =8.60 Henderson equation: pH = pKa +…

Q: What is the pH of a buffer made from 0.180 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

Q: Calculate the pH of a buffer solution made from 1.000 g of sodium chlorate NaClO3 and 0.9561 g of…

A: Write the expression for pH. pH = pKa + log[salt][acid] Here, pKa is the negative logarithm of acid…

Q: 12 a C Consider a buffer made by adding 132.8 g of NaC,H₂O₂ to 300.0 mL of 1.51 M HC₂H₂O₂ (Ka = 6.3…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base. It…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HCNO (Ka = 3.5…

A: Step 1: Step 2: Step 3: Step 4:

Q: How many grams of dry NH4 Cl need to be added to 2.10 L of a 0.100 M solution of ammonia, NH3, to…

A: Given: Volume of ammonia solution = 2.10 L Molarity of ammonia solution = 0.100 M pH of buffer…

Q: What is the pH of a buffer made by combining 45.0 mL of 0.150 M nitrous acid and 20.0 mL of 0.175 M…

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.160 mol of KBrO in…

A: For HBrO , pKa = -log Ka = -log ( 2.5 × 10⁻⁹ ) = 9 - log2.5 = 9 - 0.40 = 8.60 For buffer : pH = pKa…

Q: a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka =…

A: Given: pH = 2.25 Concentration of HClO2 = 0.100 M Volume of HClO2 = 500.00 mL Concentration of NaOH…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HOCl (Ka = 3.5…

A: 1. **Understand the problem and what we're trying to achieve:** - We have a solution of HOCl, a…

Q: A 200mL solution of 0.3 M weak acid is titrated with 40 mL of 1.5 M NaOH. If the Ka of the acid is…

A: Number of mmoles of HA = Molarity x volume (mL) = 0.3 x 200 = 60 mmoles Number of moles of NaOH =…

Q: Calculate the pH of a buffer system containing 0.25 M HF and 0.5 M NaF. (Ka for HF is 7.1 x 10-4).

A: The acid ionization constant for HF is 7.1×10 -4. pKa = -log Ka = -log (7.1×10-4)=3.1

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

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 To Calculate

VIEW

Step 2 Formula used and Calculation

VIEW

Step 3 Conclusion

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.
A buffer solution is prepared by dissolving 0.10 mol of acetic acid and 0.10 mol of sodium acetate in 1 L of solution. A 10-mL portion of 1 M HCl is then added to the solution. How much does the addition change the pH of the buffer? [Ka (CH3COOH) = 1.8 x 10-5]
Draw the structures for the following compounds 1. 4-(1-methylethyl)heptane 2. 5-(1,1-dimethylethyl)nonane 3. ethylcyclobutane
What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)
What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in 2.0 L of solution?
How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.40? (Ka for HF is 6.8 × 10⁻⁴)
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.150 mol of KBrO in 2.0 L of solution?
The acid HX has a pKa of 5.76. What volume, in mL, of a 0.100 M solution of sodium hydroxide needs to be added to 25.00 mL of a 0.100 M solution of the acid solution to make a buffer with a pH of 5.44?
How many grams of KClO needed to mix with 120.0 mL of 0.240 M HClO (ka=2.90 ×10-8), to make a buffer with a pH of 8.00
How many grams of sodium hypochlorite, NaCIO, need to be added to 227 mL of a 0.185 M solution of hypochlorous acid, HCIO, to get a buffer with a pH of 7.92? The Ką for hypochlorous acid is 2.9 × 10-8.