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October 1, 2014

October 1, 2014

Posted by **djella** on Tuesday, October 25, 2011 at 10:55pm.

2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH solution?

3. a 0.481 gram sample of an unknown acid (HX) required 28.95 mL of 0.2103 M NaOH for neutralization to a phenolphthalein endpoit. What is the molar mass of the acid?

4. what volume of 0.1037 M HCL is necessary to neutralize 0.3643 grams Ca(OH)2? included a balanced equation?

5.calculate the molar concentration of propionic acid (HC3H5O2) in solution if 10.00mL of a propionic acid solution is neutralized with 16.85mL of 0.143 M NaOH solution.

6. calculate the mass percent of propionic acid (HC3H5O2) in solution. (Assume the density of the solution to be 1.00g/mL.)

- chemistry -
**DrBob222**, Tuesday, October 25, 2011 at 11:16pmYou fare better if you post one question per try.

1.

M1 x mL1 = M2 x mL2

2.

Since NaOH and HCl react 1:1 (write the balanced equation to see that), then

mLHCl x MHCl = mLNaOH x M NaOH

3.

moles NaOH = M x L = ?

moles HX = the same

moles HX = grams/molar mass

Solve for molar mass.

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