Question

Part II. pH of a series of hydrochloric acid solutions. Obtain 10.0 mL of 0.10 M...

Part II. pH of a series of hydrochloric acid solutions.

Obtain 10.0 mL of 0.10 M hydrochloric acid Predict the value of the pH. Measure the pH with the pH meter. Record the value.

Take 1.00 mL of the 0.10 M HCl(aq) in the previous step, and put it in another clean beaker. Add 9.00 mL of deionized water and stir. What is the new concentration of HCl(aq)? Predict the pH. Measure the pH. Record the value.

Add 90.0 mL of deionized water to the diluted HCl in step 2. What is the new concentration of HCl(aq)? Predict the pH. Measure the pH. Record the value.

Part III. pH of acetic acid solutions. Remember, acetic acid is a weak acid, with a Ka = 1.8 x 10−5.

Obtain 10.0 mL of 0.10 M acetic acid and place in a clean dry 50.0 mL beaker. Predict the value of the pH. Measure the pH with the pH meter. Record the value.

Take 1.00 mL of the 0.10 M CH3COOH(aq) in the previous step, and put it in another clean beaker. Add 9.00 mL of deionized water and stir. What is the new concentration of CH3COOH(aq)? Predict the pH. Measure the pH. Record the value.

Add 90.0 mL of deionized water to the diluted CH3COOH(aq) in step 2. What is the new concentration of CH3COOH(aq)? Predict the pH. Measure the pH. Record the value.

Homework Answers

Answer #1

Solved the complete Part 2 with multiple steps, post multiple question to get the remaining answers

Part 2

a) HCl is a strong acid, hence it will dissociate completely forming H+ and Cl-

pH = -log[H+] = -log[0.10] = 1

b) Adding 1 mL HCl to 9 mL of water

Final molarity of HCl = Initial Molarity of HCl * (Volume of HCl/Volume of HCl + Volume of water)

=> 0.1 * 1/(1+9) = 0.01M

pH = -log[H+] = -log(0.01) = 2

c) Initially we have 10mL of 0.01M HCl and this solution we are adding 90mL of H2O

Final molarity of HCl = Initial Molarity of HCl * (Volume of HCl/Volume of HCl + Volume of water)

=> 0.01 * 10/(10+90) = 0.001M

pH = -log[H+] = -log(0.001) = 3

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations...
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that “one solution is a buffer” is not sufficient....
Calculate pH of 0.10 M hydrochloric acid (why no Ka?) Calculate the pH of a 0.100...
Calculate pH of 0.10 M hydrochloric acid (why no Ka?) Calculate the pH of a 0.100 M calcium hydroxide (hint: write the formula first & rxn in water) Calculate the pH and % ionization of a 0.05 M hydrofluoric acid (ka = 8.0 x 10 -4) . What is the hydrogen ion concentration for a hydrochloric acid solution that has a pH of 2.30?
A beaker with 1.90×102 mL of an acetic acid buffer with a pH of 5.000 is...
A beaker with 1.90×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 9.00 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( − ) sign if the pH has...
A beaker with 2.00×102 mL of an acetic acid buffer with a pH of 5.000 is...
A beaker with 2.00×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 9.00 mL of a 0.330 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( − ) sign if the pH has...
What is the theoretical pH of 0.10 M Acetic Acid with the addition of HCl? 1.00...
What is the theoretical pH of 0.10 M Acetic Acid with the addition of HCl? 1.00 ml of 1.0 M Hcl was added to the acetic acid solution. calculate the molarities of the acetic acid and hcl in the 51.0ml solution and calculate the theoretical pH of the solution.
Part A A beaker with 135 mL of an acetic acid buffer with a pH of...
Part A A beaker with 135 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 4.30 mL of a 0.400 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( − ) sign if the...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared....
A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Calculate the pH when 21.1 mL of 0.014 M HCl is added to 100.0 mL of the above buffer.
Part A A beaker with 135 mL of an acetic acid buffer with a pH of...
Part A A beaker with 135 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.30 mL of a 0.450 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( − ) sign if the...
You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 4.90...
You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 4.90 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76), 3.00 M NaOH, and water. Answer the following questions regarding the preparation of the buffer. 1. How many grams of acetic acid will you need to prepare the 500 mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. 2. What volume of 3.00 M NaOH must...