Answered: What quantity in moles of HCl need to…

What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 3.60? (Ka for HF is 6.8 x 10-4)

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 student needs to prepare a buffer made from HF and KF with pH 3.428. If Ka for HF is 7.20 × 10-4,…

Q: Calculate the pH of a buffer that is 0.10 M HF and 0.080 M NaF. The Ka for HF is 3.5 x 10-4.

A: pKa of the buffer solution has to be determined for calculating the pH of the solution.

Q: What quantity in moles of CH3NH3CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH₂ (Kb…

A: To calculate the number of moles of salt needed to prepare a buffer of given pH

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 quantity in moles of HCI need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: Given:pH of buffer solution = 3.00Ka for HF = 6.8×10−4 The pKa for HF is calculated as:pKa=−logKa…

Q: How many grams of solid potassium fluoride should be added to 1.00 L of a 0.140 M hydrofluoric acid…

A: Given -Volume= 1.00L Concentration of hydrofluoric acid= 0.140 M pH= 4.097 Ka(HF)=7.20×10-4Mass of…

Q: Calculate the mass of C5H5NHCI (molar mass = 113.56 g/mol) that must be added to 0.80 L of 2.5 M…

A: Given, Kb of C5H5N( weak base) is 1.8 X 10-9Therefore, pKb = - log(Kb) =…

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: 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: How many moles of solid NaF would have to be added to 1.0 L of 1.85 M HF solution to achieve a…

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: 1.0 L of acetate buffer is made by combining 0.50 M CH3COOH with 0.50 M CH3COONa. The Ka of CH3COOH…

Q: How many grams of solid sodium fluoride should be added to 2.00 L of a 0.175 M hydrofluoric acid…

A: Given - Volume= 2.00L Concentration of hydrofluoric= 0.175M pH=2.271 Ka(HF)=7.20×10-4 Mass=?

Q: What concentration of HF do you need to add to a 0.35 M NaF solution to get a buffer solution pH of…

A: Using the Henderson Hasselbach equation: pH=pKa + log[conjugate base][weak acid] Dissociation of…

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: 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: 2. Phenol (C6H5OH) has a Ka of 1.6*10-10. Starting with a 100.0 mL solution that is 0.300 M phenol,…

A: Given that : Volume of C6H5OH=100mLIts concentration=0.300 MpH = 10Ka of C6H5OH=1.6×10-10So,…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: Salt of strong acid and strong base are neutral Salt of strong acid and weak base is acedic and…

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: 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: A buffer is prepared by mixing 206 mL of 0.452 M HCl and 0.500 L of 0.400 M sodium acetate,…

A: Given: Molarity of HCl = 0.452 M Volume of HCl = 206 mL Molarity of sodium acetate = 0.400 M Volume…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.80 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: Given data is as follows: The pH of the buffer solution = 9.80 The Ka of HCN = 4.9×10-10 The ratio…

Q: Calculate the pH of a solution that is 0.20 M HOC1 and 0.92 M KOCI. Ka = 3.5x10-8 pH = 8.16 b In…

Q: How many millilitres of a 0.1 M solution of NaF and of 0.1 M solution of HF must be mixed to obtain…

A: Acidic buffer :- A mixture of weak acid and its salt with strong base is known as acidic buffer For…

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

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

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

A: moles of HCl added to prepare the buffer solution

Q: what is the pH of a buffer solution that contains 0.100M HF and 0.120 M NaF? The Ka of HF is…

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: What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: Buffer solution made of a mixture of weak acid and its conjugate base salt in aqueous…

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

Q: what volume of Boric acid 0.1 M and what volume of sodium hydroxide 0.1 M should be added together…

A: Step 1: Here, the amount of desired buffer solution is not given so it should be assumed as 100mL (…

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

A: Given data isvolume of NaF solution = 200.0 mLMolarity of NaF solution = 0.200 MpH of the buffer =…

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

What quantity in moles of HCl need to
be added to 200.0 mL of a 0.200 M
solution of NaF to make a buffer with a
pH of 3.60? (Ka for HF is 6.8 × 10-4)

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: Introduction to problem:

VIEW

Step 2: Calculation part:

VIEW

Step 3: Further calculation:

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 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

Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate, NaC3H5O3 if 9.474 mL of 4.192 M NaOH is added. The total volume is 1.00 L. The Ka for lactic acid is 1.4*10-4.
How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850? Mass= g
a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH = b) Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration = M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka value of HA ? = d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH = 50.0 mL pH =
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.
What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 1010)
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.
Give only typing answer with explanation and conclusion
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.