In: Chemistry

A solution of 0.2152M NaOH is used to neutralize 15.00mL H2SO4
solution.

H2SO4(*a**q*) + 2NaOH(*a**q*) ?
Na2SO4(*a**q*) + 2H2O(*l*)

If 32.59mL NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution?

H2SO4(*a**q*) + 2NaOH(*a**q*) ?
Na2SO4(*a**q*) + 2H2O(*l*)

Acid Base

M_{1}
=
M_{2} =0.2152M

V_{1 } = 15ml
V_{2} =32.59 ml

n_{1} = 1
n_{1} =2

M1V1 M2V2

n_{1 }
n2

M1 = M2V2n1/n2V1

= 0.2152*32.59*1/2*15 = 0.2337M

13. A 15.0 mL NaOH solution is required to neutralize
10.0 mL of 0.100 M H2SO4(aq)
solution.
What is the concentration
of NaOH solution used?
2NaOH (aq) + H2SO4(aq) → Na2SO4(aq) +
2H2O(l)

Answer the following questions for the reaction
NiCl2(aq)+2NaOH(aq)→Ni(OH)2(s)+2NaCl(aq)
A.How many milliliters of 0.200 M NaOH solution are
needed to react with 42.0 mL of a 0.320 M NiCl2
solution?
Express your answer with the appropriate units.
B.How many grams of Ni(OH)2 are produced from the reaction of
51.0 mL of a 2.00 M NaOH solution and excess NiCl2?
Express your answer with the appropriate units.
C.What is the molarity of 30.0 mL of a NiCl2 solution that
reacts completely with...

1. Calculate the molar amount of KHP used to neutralize the NaOH
solution.
2. Calculate the molar concentration of the NaOH solution that
you prepared.
3. Compare the actual molarity of your NaOH solution with your
goal of 0.10 M.
Equivalance
point-25.3,
Measurements found in lab.
Mass of NaOH
needed=0.40g
Mass of KHP needed=0.505g

Suppose it took 17.38 mL of 0.098 M NAOH solution to neutralize
the acid solution and that you used 0.77 g of green crystals to
prepare the original 50.0 mL solution (of which only 10.00 mL is
analyzed for Co at a time). Calculate the mass of cobalt in the
sample, the percent cobalt and the percent error. Thank you!

Using the above sodium hydroxide solution, 27.21 mL of the NaOH
solution is required to neutralize a volume of 28.45 mL of an
acetic acid solution having an unknown concentration to a
phenolphthalein end point. Determine the concentration, in
molarity, of the acidic solution. Start with a balanced
equation.

1. What is the molarity of a solution of NaOH if 23.4 mL
required to neutralize 25 mL of 0.25M H2SO4?
2.What is the pH of a solution produced by dissolving 1.5g HCI
to make 1L of solution?
Please help, step by step solutions .. thanks!

what is the molarity of a NaOH solution if 26.50 mL of its required
to neutralize .4150 g of pure KHP?

Balance the following eqautions:
Fe(s) + S(s) -> FeS(s)
H2SO4(aq) + NaOH(aq) ->
Na2SO4(aq) +
H2O(I)
Cu(s) + O2(g) ->
Cu2O(s)
FeCl3(aq) + NaOH(aq) ->
Fe(OH)3(s) + NaCl(aq)

Calculate the volume, in milliliters, of a 0.216 M NaOH solution
that will completely neutralize each of the following: 1.) 3.71 mL
of a 1.32 M HNO3 solution. 2.) 8.10 mL of a 0.800 M H3PO4
solution.

A solution of 0.312 M KOH is used to neutralize 15.0mL of an HF
solution If 28.3 mL of KOH is required to reach the end point, what
is the morality of HF solution.

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