Question

1) A 21.30 mL volume of 0.0975 M NaOH was used to titrate 25.0 mL of...

1)

A 21.30 mL volume of 0.0975 M NaOH was used to titrate 25.0 mL of a weak monoprotic acid solution to the stoichiometric point. Determine the molar concentration of the weak acid solution.

2.08 M

0.114 M

0.0831 M

0.00390 M

2.44 M

2)

For a weak acid (CH3COOH) that is titrated with a strong base (NaOH), what species (ions/molecules) are present in the solution at the stoichiometric point?

CH3COO-

H2O

Na+

NaCl

HCl

Homework Answers

Answer #1

1)

we have the Balanced chemical equation as:

NaOH + HA ---> NaA + H2O

Here:

M(NaOH)=0.0975 M

V(NaOH)=21.3 mL

V(HA)=25.0 mL

According to balanced reaction:

1*number of mol of NaOH =1*number of mol of HA

1*M(NaOH)*V(NaOH) =1*M(HA)*V(HA)

1*0.0975*21.3 = 1*M(HA)*25.0

M(HA) = 0.0831 M

Answer: 0.0831 M

2)

CH3COOH and NaOH react to form CH3COONa and H2O

CH3COONa is CH3COO- and Na+

CH3COO-

Na+

H2O

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
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
a. You titrate 25.0 mL of 0.60 M NH3 with 0.60 M HCl. Calculate the pH...
a. You titrate 25.0 mL of 0.60 M NH3 with 0.60 M HCl. Calculate the pH of the solution after adding 5.00, 15.0, 22.0, and 30.0 mL of the acid. Ka = 5.6×10-10 pH(5.00 mL added) ------------------------------ pH(15.0 mL added)------------------------------ pH(22.0 mL added) ---------------------------- pH(30.0 mL added)---------------------------- b. itration of 27.9 mL of a solution of the weak base aniline, C6H5NH2, requires 28.64 mL of 0.160 M HCl to reach the equivalence point. C6H5NH2(aq) + H3O+(aq) ⇆ C6H5NH3+(aq) + H2O(ℓ)...
If   14.99 mL of NaOH are required to titrate 15.00 mL of a   0.46 M oxalic acid solution,...
If   14.99 mL of NaOH are required to titrate 15.00 mL of a   0.46 M oxalic acid solution, what is the concentration of the NaOH? A solution of a theoretical triprotic acid was prepared by dissolving 4.980 g of solid in enough DI water to make 500.0 mL of solution.   10.10 mL of a 0.448 M solution was required to titrate 20.00 mL of this acid's solution. 1. What is the concentration of the acid solution? 2. What is the molar mass...
A titration is done using a 0.1302 M NaOH solution to determine the molar mass of...
A titration is done using a 0.1302 M NaOH solution to determine the molar mass of a monoprotic weak acid (HA). If 50.00 mL of a 1.863 g sample of the unknown acid (HA) is titrated to the equivalence point/end point with 70.11 mL of a 0.1302 M NaOH aqueous solution, what is the molar mass of the unknown acid?
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of 0.1 M H3PO4? Question options: a) V = 12 mL b) V = 6 mL c) V = 18 mL d) V = 30 mL he pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x 10-7) is titrated with a 0.20 M strong acid is: Question options: a) pH = 2.9 b) pH = 1.7 c) pH =...
to what volume should you dilute 50.0 mL of 5.00 M NaOH solution so that 25.0...
to what volume should you dilute 50.0 mL of 5.00 M NaOH solution so that 25.0 mL of this diluted solution requires 28.5 mL of 1.50 M HCl solution to titrate?
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL...
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL of H2SO4 are needed to reach the end point. 2.  If 35.00 mL of 0.0200 M aqueous HCl is required to titrate 30.00 mL of an aqueous solution of NaOH to the equivalence point, the molarity of the NaOH solution is ________ 1 M.
Initial NaOH volume mL Final NaOH volume mL Total volume of NaOH used mL 9 0...
Initial NaOH volume mL Final NaOH volume mL Total volume of NaOH used mL 9 0 9 9 0.2 8.8 9 0.3 8.7 Three trials, average volume of NaOH used mL = 8.8 Average volume of NaOH used mL Concentration CH3COOH in vinegar mol/L % CH3COOH in vinegar 8.8 72 83 1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer...
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX,...
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX, a weak monoprotic acid, the pH of the resulting solution is 3.74. Calculate the Ka of the acid. 2. Will the equivalence point of ammonia plus HCl be higher, lower, or equal to 7? Explain.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT