16.17 Calculate the pH of the 0.20 M NH3/0.20 M NHẠCIbuffer. What is the pH of the buffer after the addi-tion of 10.0 mL of 0.10 M HCl to 65.0 mL of thebuffer?

Answered: Image /qna-images/answer/79d3795f-5173-4fbc-8e97-7c7c17a110cf.jpg

Answered: 16.17 Calculate the pH of the 0.20 M…

16.17 Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl buffer. What is the pH of the buffer after the addi- tion of 10.0 mL of 0.10 M HCl to 65.0 mL of the buffer?

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 290.0-mL buffer solution is 0.300 mol/L in acetic acid and 0.300 mol/L in sodium acetate.…

Q: 5.)20.0 ml of 0.200M hypobromous acid, HBrO, is titrated with 0.250M sodium hydroxide, NaOH.…

A: Volume of HBrO = 20 mL Molarity of HBrO = 0.200 M Molarity of NaOH = 0.250 M To determine pH at…

Q: buffer solution contains 0.250 mol of HF and 0.650 mol of NaF in 1.00 L of solution. What is the…

Q: What is the pH of a 498.2mL buffer solution with 0.239M HF and 66.55 grams of potassium fluoride?…

Q: (a) Calculate the pH of a buffer solution containing 0.40 mole of KF and 0.50 mol of HF in 1.50…

A: pH of buffer solution is calculated using Henderson–Hasselbalch equation, amount of strong acid HCl…

Q: A chemistry graduate student is given 300. mL of a 0.20M hydrocyanic acid (HCN) solution.…

A: The Henderson-Hasselbalch equation gives the pH of buffer solution it is mathematically represented…

Q: The bicarbonate/ carbonic acid buffer is of extreme importance to our bodies. The pH of importance…

Q: How many moles of sodium hydroxide would have to be added to 250 mL of a 0.385 M hypochlorous acid…

A: The volume of hypochlorous acid = 250 mL The molarity of hypochlorous acid = 0.385 M pH of buffer to…

Q: When a 27.5 mL sample of a 0.477 M aqueous hydrocyanic acid solution is titrated with a 0.371 M…

A: Given : Concentration of HCN = 0.477 M Concentration of Ba(OH)2= 0.371 M Volume of HCN = 27.5 mL…

Q: 40 mL of NaOH solution with unknown concentration is titrated with 0.10 M of CH3COOH solution in the…

A: From the given data we haveVolume of NaOH (V1)=40mlMolarity of NaOH (M1)=?Volume of…

Q: 16.13 The pH of a bicarbonate-carbonic acid buffer is 8.00. Calculate the ratio of the concentration…

A: Here we have to determine ratio of concentration of carbonic acid to bicarbonate ion in buffer…

Q: 16.13 The pH of a bicarbonate-carbonic acid buffer is 8.00. Calculate the ratio of the concentration…

Q: 13. 30 ml of 0.20 M NH,OH & 25 ml of 0.20 HCl are mixed. What is the pH? K = 1.8 X 10% Calculate the…

A: NH4OH is weak base and when it combines with limiting strong acid, HCl then a basic buffer is…

Q: None

A: Step 1:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Acetic acid has a Ka of 1.8×10−5. a.) What is the pH of a buffer solution containing 0.20 M HC2H3O2…

A: Concentration of acetic acid[C2H3O2] = 0.20 MConcentration of acetate ion = 0.13 MKa = 1.8*10-5pH =…

Q: A chemistry graduate student is given 500. mL of a 0.50M chlorous acid (HCIO) solution. Chlorous…

Q: Suppose you want to make 500 mL of a 0.20 M Tris buffer at pH 8.0. On the shelf in your lab, you see…

A: According to the question we have, The pKa of tris is given by = 8.06 The molar concentration of…

Q: You need to prepare an acetate buffer of pH 5.45 from a 0.654 M acetic acid solution and a 2.53 M…

A: The number of moles of acetic acid (nAcOH) in 480 mL 0.654 M solution is calculated using equation…

Q: A chemistry graduate student is given 300. mL of a 1.20M nitrous acid (HNO2) solution. Nitrous acid…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.90 buffer? (Ka of HCN is 4.9 × 10-10)

Q: Calculate the pH at the equivalence point for the fol- lowing titration: 0.10 M HCOOH versus 0.10 M…

A: Given: Concentration of HCOOH = 0.10 M And concentration of NaOH = 0.10 M The titration reaction…

Q: Assume that 32.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a…

A: Acid and base react with each other to form salt and water. The nature of salt depends on the nature…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and…

A: Let y mL benzoic acid and (100 – y) mL sodium benzoate are mixed. For acidic buffer solution, pH =…

Q: suppose that the ph of buffer A turned out at ph 5.5 instead of ph 5.0 (100.0 mL of a 0.5 M buffer)…

A: Buffer solution is defined as a solution which resists any change in its pH value even when small…

Q: 2. If 5.0 mL of 0.010 M NaOH is added to 100 mL of the buffer in Problem 1, how much will the pH…

Q: One of the factors that can affect the pH of a buffered solution is the molar ratio of the conjugate…

Q: You need to prepare an acetate buffer of pH 5.42 from a 0.647 M acetic acid solution and a 2.43 M…

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

Q: Titration curves. Plot a titration curve for the given acid-base titration. Determine at least 5…

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

Q: Which of the following buffering systems would work best for a laboratory experiment requiring a pH…

A: The objective of this question is to identify the best buffering system for a laboratory experiment…

Q: How many grams of solid calcium cyanide, Ca(CN)₂ must be added to 400.0 ml of 0.350M hydrocyanic…

A: Henderson-Hasselbalch equation is used for the pH of buffer solution. pH=pKa +logconjugate baseweak…

Q: a) A chemist prepares a buffer solution by mixing 60.0 mL of 0.150 M NHs and 50.0 mL of 0.100 M…

Q: A chemistry graduate student is given 300. mL of a 0.20M hydrocyanic acid (HCN) solution.…

Q: A buffer solution is 0.422 M in HCN and 0.268 M in NaCN . If Ka for HCN is 4.0×10-10 , what is the…

A: Calculate the value of pKa:

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: pH

Q: A buffer solution of 200 mL is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX.…

A: Buffer solution :- A solution which resists change in its pH value by the addition small amount of…

Q: A student is asked to prepare a buffer solution at pH = 8.60, using one of the following weak acids:…

A: Given : pH = 8.60

Q: Assume that you prepare a buffer by mixing 37 ml of 0.26 M acetic acid and 53 ml of 0.15 M sodium…

A: We have to calculate pH of the buffer solution

Q: What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H30₂) and 20.0 g of sodium…

A: To determine pH of buffer solution Henderson Equation can be used depending on the type of buffer…

Q: What is the pH of buffer solution containing 0.25 M acetic acid and 0.4 M sodium acetate ?

A: Answer:- this question is answered by using the simple concept of calculation of pH of a buffer…

Q: Calculate the pOH of 103.16 mL of a buffer initially consisting of 0.1752 M H2NCH2COOH and 0.1573 M…

Q: When a 16.9 mL sample of a 0.317 M aqueous acetic acid solution is titrated with a 0.391 M aqueous…

A: As we start the titration there will be a acidic buffer established due to presence of weak acid and…

Q: 4- Which of the following mixtures is a buffer and calculate its pH: (K=1.8 × 10) a- 25ml 0.1M HCl…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

16.17 Calculate the pH of the 0.20 M NH3/0.20 M NHẠCI
buffer. What is the pH of the buffer after the addi-
tion of 10.0 mL of 0.10 M HCl to 65.0 mL of the
buffer?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

There are 250 ml of a Buffer solution, where the concentration is 0.225 M of acetate of sodium and 0.225 M acetic acid. What will be the change in pH if 300 ml of a 0.18 M HCl solution?
Calculate the mass of ammonium chloride that must be added to 500.0 mL of 0.52 M NH3 to prepare a pH 8.50 buffer.
Cacodylic acid (dimethylarsinic acid, HASO2(CH3)2) is a common buffer used in biology to prepare and fix biological samples. The pKa of cacodylic acid is 6.3. Part A What is the pH of a buffer solution prepared by mixing 20.0 mL of 0.0600 mol L-'NaOH with 20.0 mL of 0.105 mol L-!cacodylic acid? Express your answer using one decimal place. femplates Symbols uado redo reset keyboard shortcuts help, pH = Submit Request Answer Part B What is the pH of the buffer solution in part A after 0.0002 moles of H30+ was added to the mixture? Express your answer using one decimal place. Templates Symbols undo redo reset keyboard shortcuts help, pH =
Subject: chemistry
For 480.0 mL of a buffer solution that is 0.120 M in HC2H3O2 and 7.50×10−2 M in NaC2H3O2 , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Ka(HC2H3O2)=1.8×10−5 .)
Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.
If 0.50 mL of 0.087 M HCl is added to the solution in (a), how many moles of the acetic acid, sodium acetate and HCI will be present after the reaction is done? What is the % pH change?
When a 29.6 mL sample of a 0.484 M aqueous hydrofluoric acid solution is titrated with a 0.499 M aqueous sodium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 43.1 mL of sodium hydroxide have been added?
What is the pH of a buffer solution that is 0.214 M in ammonia and 0.390 M in ammonium chloride (NH4CI)? The Kü of ammonia is 1.8 x 10-5. (Two decimal places)
Determine the volume of 0.10 M CH3COOH and 0.10 M CH3COONa required to prepare 10.0 mL of buffer of each of the following three pH values: 1.) pH 3.7 2.) pH 4.7 3.) pH 5.7
How many moles of sodium hydroxide would have to be added to 125 mL of a 0.376 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.050? moles
16.11 Calculate the pH of the buffer system made up of 0.15 M NH3/0.35 M NH4Cl.