How did they get these answers? How much volume of 0.2 M NaOH should be added...

Question

Question

How did they get these answers?

Answer 1

Answer #1

12) At equivalence point,

M1V1 = M2V2 [ M1,V1 refers to HCl and M2,V2 refers to NaOH ]

0.1 M x 30 mL = 0.2 M x V2

V2 = 0.1 M x 30 mL/ 0.2 M

= 15 mL

V2 = 15 mL

Therefore, volume of NaOH should be added = 15 mL

13)

[HCl ] = [H+] = 0.1 M x 30 mL = 3 mmol

[NaOH ] = [OH-] = 0.2 M x 15 mL = 3 mmol

Hence [H+] = [OH-],

this is the equivalence point and

thus,

pH = 7.0

Add a comment

Answer 2

Similar Homework Help Questions

PROCESSING THE DATA 1. COMPLETE DATA TABLE 2. Determine the volume of NaQH added at the...

PROCESSING THE DATA 1. COMPLETE DATA TABLE 2. Determine the volume of NaQH added at the equivalence point. 3. Calculate the number of moles of NaOH used. 4. See the equation for the neutralization reaction given in the introduction. Determine the number of moles of HCl used. 5. Recall that you pipeted out 10.0 mL of the unknown HCl solution for the titration. Calculate the HCl concentration. Trail 1 Trial 2 Concentration of NaQH 0.1 M 0 ml NaQH volume...
How much volume of a 0.102 M NaOH solution must be added to 25.00 ml of...

How much volume of a 0.102 M NaOH solution must be added to 25.00 ml of a 0.075 M solution of benzene-1,2,3-tricarboxylic acid to obtain a pH equal to 4.80? pKa values: pKa1 = 2.86, pka2 = 4.30 and pka3 = 6.28.
6. How many mL of 0.2 M sodium acetate should be added to 200 mL of...

6. How many mL of 0.2 M sodium acetate should be added to 200 mL of 0.2 M acetic acid to make a buffer of pH 5.5? (refer to Table 2-2 on page 60 for pKa values). What is the molarity of the resulting buffer with respect to acetate (acetate + acetic acid)? 7. How many mL of 0.2 M HCl should be added to 50 mL of 0.2 M Tris base (Trishydroxymethyl aminomethane) to make a buffer of pH...

How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing...

How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing 12.212g of benzoic acid (F.W. 122.12g ; Ka = 6.28 x 10-5) to get a pH of 4.8?
A volume of 500.0 mL of 0.160 M NaOH is added to 575 mL of 0.200...

A volume of 500.0 mL of 0.160 M NaOH is added to 575 mL of 0.200 M weak acid (K, the resulting buffer? 5.93 x 10). What is the pH of HA (aq) +OH (aq)HO) + A (aq) pH = QuestronT orA Calculate the pH of the resulting solution if 35.0 mL of 0.350 M HCl(aq) is added to 45.0 mL of 0.350 M NaOH(aq). pH Calculate the pH of the resulting solution if 35.0 mL of 0.350 M HCI(aq)...
Volume NaOH added Moles of NaOH added 0.00010 Concentration of NaOH-0.1 M Concentration of HC H10.-01 M a) What is...

Volume NaOH added Moles of NaOH added 0.00010 Concentration of NaOH-0.1 M Concentration of HC H10.-01 M a) What is the pH at equivalence point? b) What is the volume of N hat equivalence point? c) Moles of NOH at the equivalence point? d) Moles of HCHO at equivalence point? e) Find K. of HC HO Find pk of HC HO 000220 ellas

When 12 mL of 0.2 M NaOH is added to 25 mL of 0.15 M HCl,...

When 12 mL of 0.2 M NaOH is added to 25 mL of 0.15 M HCl, what is the pH of the solution? When 12 mL of 0.2 M NaOH is added to 25 mL of 0.15 M acetic acid, would this solution be considered a buffer? Explain your answer. What is the pH of the solution in number 2?
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa)...

4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....

1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...

24A) 40mL of 0.2 M formic acid is titrated with a strong base (NaOH= 0.5 M). Determine the pH before any base has been...

24A) 40mL of 0.2 M formic acid is titrated with a strong base (NaOH= 0.5 M). Determine the pH before any base has been added. Please show steps and please explain why the answer is what it is. 24B) The 40mL 0.2 M formic acid is titrated with a 6.0mL of strong base. Here NaOH can be treated as a conjugate base and formic acid is the acid. please show steps and explain! Us (24-25, Acid/base, aqueous equilibrium) 24A) (4...