Question

- UR 10-M 1.0*10 (iv) lemon juice, 4.0 x 10WM. 11.123 Calculate the volume, in milliliters, of a 0.150 he volume, in millier
0 0
Add a comment Improve this question Transcribed image text
Answer #1

Question 11.123.

Formula: MaVa = MbVb

Where Ma and Mb are the molar concentrations of acid (HCl) and base (NaOH), respectively.

Va and Vb are the volumes of acid and base solutions, respectively.

i.e. 0.288 M * 25 mL = 0.150 M * Vb

Therefore, the required volume of the base (Vb) = 48 mL

Add a comment
Know the answer?
Add Answer to:
- UR 10-M 1.0*10 (iv) lemon juice, 4.0 x 10"WM. 11.123 Calculate the volume, in milliliters,...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • *Calculate the volume, in milliliters, of a 0.205 M solution of NaOH that will completely neutralize...

    *Calculate the volume, in milliliters, of a 0.205 M solution of NaOH that will completely neutralize each of the following. A- 2.40 mL of a 0.835 M solution of H2SO4. B-3.83 mL of a 1.35 M solution of HNO3. C-6.00 mL of a 3.25 M solution of HCl. *A 0.210 M NaOH solution is used to titrate 28.0 mL of a solution of H2SO4. H2SO4(aq)+2NaOH(aq)→H2O(l)+Na2SO4(aq) A-If 42.6 mL of the NaOH solution is required, what is the molarity of the...

  • 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)...

  • A volume of 500.0 mL of 0.150 M NaOH is added to 615 mL of 0.250...

    A volume of 500.0 mL of 0.150 M NaOH is added to 615 mL of 0.250 M weak acid (Kg = 4.65 x 10-'). What is the pH of the resulting buffer? HA(aq) + OH(aq) — H,O(l) + A (aq) pH If a buffer solution is 0.230 M in a weak acid (K, = 9.0 x 10-) and 0.460 M in its conjugate base, what is the pH? pH =

  • 6.What is the pH of a solution with [OH-] = 1.7 x 10-3M? 7.Calculate [H3O+] of...

    6.What is the pH of a solution with [OH-] = 1.7 x 10-3M? 7.Calculate [H3O+] of a solution with a pH of 5.5 8. A 15.0 mL sample of H2SO4solution is titrated with 24.0 mL of 0.245 M NaOH solution. What is the molarity of the H2SO4solution?H2SO4(aq) + 2 NaOH (aq) →2 H2O (l) + Na2SO4(aq)

  • 1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2...

    1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...

  • A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the...

    A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 MM CH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 15.0 mL of NaOH. and Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pH of 2.80. You have in front...

  • a. Calculate the pH of the solution if 2.3 x 10-3 moles of Sr(OH)2 is dissolved...

    a. Calculate the pH of the solution if 2.3 x 10-3 moles of Sr(OH)2 is dissolved in 250 mL of water? b. Calculate the pH of a 3.0000 M solution of NaOH? c. Calculate the pH if 6.5 g of HCl(g) are dissolved in 200 mL of water?

  • Calculate the pH in a 0.010-M solution of caffeine: C8H10N4O2(aq)+H2O(l) ⇌ C8H10N4O2H+(aq)+OH−(aq) (Hint: pKb=10.4). In a...

    Calculate the pH in a 0.010-M solution of caffeine: C8H10N4O2(aq)+H2O(l) ⇌ C8H10N4O2H+(aq)+OH−(aq) (Hint: pKb=10.4). In a titration where the original solution, was 50mL of 0.1M HCl,. What is the pH of this solution after 55 mL of 01 M NaOH(s) has been addided? Consider a buffer solution prepared from 0.3 M ethanoic acid and 0.3 M sodium ethanoate. In what ratio should the ethanoic acid be mixed with the sodium ethanoate to give a buffer solution of pH 5.6? Ka...

  • IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10)...

    IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10) solution is titrated with 0.200 M NaOH. Find the pH before titration and after 25 mL, 50 mL, and 60 mL of NaOH has been added.

  • 1. Calculate pH and % ionization of 0.25 M Naco (Ka (HCO2H) 1.8 x 10") 2-...

    1. Calculate pH and % ionization of 0.25 M Naco (Ka (HCO2H) 1.8 x 10") 2- Calculate the pH of: a) 0.35 M HNO b) 0.15 M Sr(O)2 c) 0.08 M Ba(CIO4)2 3- Calculate the pH of 0.375 L buffer solution made of a 0.18 M Acetic acid HC2H:02(Ka 1.8x 10) and a 0.134 M Potassium acetate KC2Hs02 (do not use more than 3 digits beyond the decimal point) a) before adding anything b) after adding 0.010 mol Ba(OH)2 c)...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT