Question

What is the molarity of an aqueous phosphoric acid solution if
10.33 mL is completely neutralized by 17.24 mL of 0.1301 *M*
NaOH? First, calculate the moles of H_{3}PO_{4} at
the dilution based on the volume and molarity of NaOH used.

Answer #1

What is the molarity of a solution that contains 0.978 grams of
H3PO4 in 60.0 mL of solution? What is the new molarity of the H3PO4
solution if the original solution is diluted by a factor of 3? How
many mL of the diluted solution could be completely neutralized by
12.5 mL of 0.545 M NaOH?

if 16.9 mL of an acetic acid (HC2H3O2) solution are completely
neutralized by 22.4 mL of 0.464 M Ba(OH)2 .
a. what is the molarity of the HC2H3O2? and
b.what is the molar concentration of barium ion in the resulting
solution?
for a I have 0.615 M of HC2H3O2
and for b I havr 20.1 M but I think its off. please help

A 25.00 mL sample of aqueous sulfuric acid of unknown
concentration is neutralized by 27.55 mL of 1.0002M NaOh
(aq).
a) Write a net ionic equation for this acid-base neutralization
reaction.
b) How many moles of NaOH did it take for the neutralization?
c) How many moles of sulfuric acid were neutralized?
d) What is the molar concentration of the sulfuric acid?

3. Calculate the concentration of the 25mL of phosphoric acid
Which is neutralized with 7.8 mL of 0.2M NaOH?

An aqueous solution of phosphoric acid, that is
2.00 percent by weight phosphoric
acid, has a density of 1.0092 g/mL. A
student determines that the freezing point of this solution is
-0.464 °C.
Based on the observed freezing point, what is the percent
ionization of the acid and the value of
Ka1? Assume that only the first
ionization of the acid is important.
Kf for H2O is 1.86 °C/m.
% ionized
= %
Ka1
=

a 25.0 mL sample of HCl is neutralized by 26.5 mL of 0.155M
NaOH. Calculate the molarity of the HCl solution. (Hint:In this
case, molarity of HCL is Ma(molarity of acid) in moles/liter of
HCl.)
HCl + NaOH
-->
NaCl
+ H2O

4. Calculate the mole fraction of phosphoric acid (H3PO4) in a
25.4% (by mass) aqueous solution. (Assume 500 mL of solution.)
Please show work

a concentrated phosphoric acid solution is 85% H3PO4
by mass and has a density of 1.69g/mL at 25°C. what is the molarity
of H3PO4?

A
sample of acetic acid (weak acid) was neutralized with .05M NaOH
solution by titration. 34 mL of NaOH had been used. Show your work.
CH3COOH + NaOH-----CH3COONa + H2O
a) Calculate how many moles of NaOH were used?
b) How many moles of aspirin were in a sample?
c) Calculate how many grams of acetic acid were in the
sample
d) When acetic acid is titrated with NaOH solution what is the
pH at the equivalence point? Circle the...

in an acid base titration, a sample of unknown concentration
phosphoric acid is analyzed by titration with a solution of sodium
hydroxide solution. In this analysis just enough sodium hydroxide
solution of known molar concentration is added to just react with
all of the phosphoric acid. When this condition has been met, the
endpoint of the titration has been reached. suppose that 26.38 mL
of a 0.100 M sodium hydroxide solution is added to a 30.00 mL
sample of the...

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