Calculate the change in pH after adding (2 g) from NaOH and molecular weight (40 g/mol) to a liter of a buffer solution consisting of acetic acid and sodium acetate at a concentration (0.2 M) of each? Pka 4.74, log3=0.48, log5-0.7

Calculate the change in pH after adding (2 g) from NaOH and molecular weight (40 g/mol) to a liter of a buffer solution consisting of acetic acid and sodium acetate at a concentration (0.2 M) of each? Pka 4.74, log3=0.48, log5-0.7

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: 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…

A: Introduction: We have to calculate number of moles of NaOH . Given : pH = 3.70 Ka= 6.8 × 10-4

Q: How many mL of 0.200 M NaOH or 0.200 M HCl must be added to a 100.0 mL buffer solution containing…

A: Molarity of NaOH = 0.200 MMolarity of HCl = 0.200 MTotal volume of buffer solution = 100.0…

Q: When a 28.1 mL sample of a 0.423 M aqueous hydrocyanic acid solution is titrated with a 0.462 M…

Q: A student needs to prepare a buffer solution with a pH of 5.73. Assuming a pKa of 4.06, how many mL…

A: Given,Molarity of NaOH = 0.1 MMolarity of acid ( HB ) = 0.1 Mvolume of HB = 15.0 mLpH of the buffer…

Q: What is the hydronium ion concentration in a buffer solution prepared by mixing 50.00 mL of 0.10 M…

Q: A buffer consists of 0.150 M acid, HA, and 0.200 M of its conjugate base, A. If HA has a K, of 4.84…

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: If you have 50.0 mL of a 0.125 M acetic acid, HC,H,O, what mass of sodium acetate, NaC,H,O,, should…

A: Given: pH of the solution= 5.25 Volume ov the solution= 50 mL=0.05 L pKa of acetic acid = 4.76…

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

Q: You have 500 mL of a buffer solution conatining 0.154 M acetic acid (CH3COOH) and 0.158 M sodium…

A: we have to calculate the pH after NaOH is added to the buffer solution

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is…

A: Given data,[HA]=0.2M[A-]=0.1MpKa=7.5Molarity of KOH=1MVolume of KOH=50mL0.05LVolume of buffer=1L

Q: A benzoic acid-sodium benzoate buffer is prepared by dissolving a certain amount of sodium benzoate,…

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

Q: A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka of the acetic acid is…

A: Calculation of pKa of acetic acid: pKa=-log Ka=-log (1.8×10-5)=4.745

Q: A buffer solution contains 0.202 M of a weak acid and 0.224 M of its conjugate base. The K, of the…

A: Buffer solution is a solution whose pH does not changes on standing as well as on addition of small…

Q: Given 100.0 mL of a buffer that is 0.50 M in HOCl and 0.60 M in NaOCl, what is the pH after 10.0 mL…

A: Given, molar concentration of weak acid, HOCl = 0.50 M Volume of buffer = 100.0 mL = 0.100 L Molar…

Q: What is the pH of a weak base-strong acid titration when 20.0 mL of 0.56 M of NaOCl (Ka = 3.0*10-8)…

Q: 15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What…

A: Molarity of NaOH=0.10 M The volume of NaOH=5 mL Molarity of HF=0.10 M The volume of HF=10 mL The…

Q: At a certain point in a titration, 25 mL of 0.1M NaOH, has been added to 40 mL of a 0.1M solution of…

A: Buffer solution is defined as an aqueous solution which have weak acid and Conjugate of Strong base.…

Q: What is the pH of the resulting buffer solution when 25mls of 0.10 M NaH is added to 25mls of 0.200…

A: pH of the buffer solution is calculated by using Henderson equation, it is,

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: 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: A buffer solution contains 0.750 mol of HF and 0.850 mol of NaF in 1.00 L of solution. What is the…

A: Given : Moles of HF = 0.750 mol. Moles of NaF = 0.850 mol. And moles of NaOH added = 0.030 mol.

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

A: We can find the volume of benzoic acid and sodium benzoate to prepare buffer solution as given…

Q: If you are going to prepare 100 ml each of the following two (2) buffers: • Buffer 1 will have a…

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

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

Q: Which of the following acids (listed with Ka values) and their conjugate base should be used to form…

A: Answer: HClO2 Amongst all options, the HClO2 acid and its conjugate is superior choice for the…

Q: When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M…

A: we need to calculate the pH for the above titration

Q: When a 20.1 mL sample of a 0.367 M aqueous hydrocyanic acid solution is titrated with a 0.492 M…

A: Answer:Number of moles of any specie in the solution is always equal to its molar concentration and…

Q: Payli

A: The objective of this question is to determine the volume of 0.100 M benzoic acid and 0.240 M sodium…

Q: Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find…

Q: Buffers will resist pH changes following the addition of acid or base within about +/-1 pH unit of…

A: Buffers are the solutions which are formed due to the presence of either weak base along with its…

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

A: Given, Volume of the buffer solution = 100.0 mL pH = 4.00 [Benzoic acid] = 0.100 M [Sodium…

Q: How many grams of sodium formate, HCOONa, are required to mix with 1.50 Liters of 0.500 M formic…

Question

Calculate the change in pH after adding (2 g) from
NaOH and molecular weight (40 g/mol) to a liter of a
buffer solution consisting of acetic acid and sodium
acetate at a concentration (0.2 M) of each?
Pka 4.74, log3–0.48, log5-0.7
а

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps

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

You have 0.100 M solutions of acetic acid ( p?a = 4.76 ) and sodium acetate. If you wanted to prepare 1.00 L of 0.100 M acetate buffer of pH 4.00 , how many milliliters of acetic acid and sodium acetate would you add?
4. 15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What is the pH of this buffer after0.30mL of 1.0 M sodium hydroxide are added to it? The Ka for HF is 6.8 x 10-4.
What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.
Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?
15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What is the pH of this buffer after 0.24 mL of 1.0 M sodium hydroxide are added to it? The Ka for HF is 6.8 x 10-4.
The following figure represents a small portion of an acetic acid-acetate buffer. (Solvent molecules have been omitted for clarity; pka of acetic acid =4.75. a) what is the pH of the buffer 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)
Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl (Correct answer) 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH please explain. thanks!
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 buffer with a pH of 3.10? (Ka for HF is 6.8 × 10⁻⁴)
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 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.