Question

What volume of a 0.50 M KOH solution is needed to neutralize
completely each of the following?

i) 10.0 mL of a 0.30 M HCl solution

ii) 15.0 mL of a 0.25 M H3PO4 solution

Answer #1

part 1

millimoles of HCl = Molarity x volume in mL = 0.3M x 10 mL = 3 mmiol

let see the balanced equation

HCl + KOH ---> KCl + H2O

1 mol of HCl required 1 mol of KOH accordingly

3 mmol of HCl required 3 mmol of KOH

mmol of KOH = 3 mmol

volume of KOH = mmol / M olarity = 3 mmol / 0.5M = 6 mL

part B

mmol of H3PO4 = 0.25 M x 15 mL = 3.75 mmol

see the balanced equation

H3PO4 + 3KOH ---> K3PO4 + 3H2O

1 mmol of H3O4 required 3 mmol of KOH accordingly

3.75 mmol required 3 x 3.75 = 11.25 mmol of KOH

volume of KOH = 11.25 / 0.5 = 22.5 mL

what is the volume, in millimeters, of a 0.350 m kOH
needed to completely neutralize 15.0 ml of a 0.250 m H2So4
solution?

What be the molarity of a KOH solution if, during a titration
with 0.50 M HCl, 34.5 mL of the HCl neutralized 22.4 mL of the KOH
solution?
a.) How much of a .50 M solution of H2SO4 would be needed to
neutralize the same amount of KOH solution?

Part A
What volume of 0.105 M HClO4 solution is needed to
neutralize 55.00 mL of 9.00×10−2M NaOH?
Part B
What volume of 0.120 M HCl is needed to neutralize 2.70
g of Mg(OH)2?
Part C
If 25.6 mL of AgNO3 is needed to precipitate all the Cl− ions in
a 0.770-mg sample of KCl (forming AgCl), what is the molarity of
the AgNO3 solution?
Part D
If 45.7 mL of 0.102 M HCl solution is needed to
neutralize a...

A) What volume of 0.150 M HClO4 solution is needed to neutralize
59.00 mL of 8.80×10−2 M NaOH? B) What volume of 0.130 M HCl is
needed to neutralize 2.87 g of Mg(OH)2? C) If 26.4 mL of AgNO3 is
needed to precipitate all the Cl− ions in a 0.755-mg sample of KCl
(forming AgCl), what is the molarity of the AgNO3 solution? D) If
45.8 mL of 0.112 M HCl solution is needed to neutralize a solution
of KOH,...

What volume of a 0.500 M HCl solution is needed to neutralize
each of the following
a. 15..0 mL of a 0.300 M NaOH solution
b. 19.0 mL of a 0.200 M Ba(OH)2 solution

a)What volume of 0.122 M HCl is needed to neutralize
2.61 g of Mg(OH)2?
b)If 25.4 mL of AgNO3 is needed to precipitate all the Cl− ions
in a 0.755-mg sample of KCl (forming AgCl), what is the molarity of
the AgNO3 solution?
C)If 45.1 mL of 0.102 M HCl solution is needed to
neutralize a solution of KOH, how many grams of KOH must be present
in the solution?

How many grams of 4.15% (w/w) solution of KOH in water is needed
to neutralize completely the acid in 13.1 mL of 0.385 M H2SO4?

Calculate the volume of
0.730-M NaOH solution needed to completely
neutralize 58.9
mL of a 0.700-M
solution of the monoprotic acid HBr.
__________ mL NaOH

(a) How many milliliters of 0.165 M HCl are needed to
neutralize completely 35.0 mL of 0.101 M
Ba(OH)2 solution?
________ ml
(b) How many milliliters of 2.50 M
H2SO4 are needed to neutralize 50.0 g of
NaOH?
_________ mL
(c) If 56.8 mL of BaCl2 solution is needed to
precipitate all the sulfate in a 544 mg sample of
Na2SO4 (forming BaSO4), what is
the molarity of the solution?
_________M
(d) If 47.5 mL of 0.250 M HCl solution...

Determine the volume (in mL) of 0.304 M KOH required to
neutralize 23.52 mL of 0.125 M H3PO4. HINT:
First write a balanced equation.

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