A solution of 0.2152M NaOH is used to neutralize 15.00mL H2SO4
solution.
H2SO4(aq) + 2NaOH(aq) ?
Na2SO4(aq) + 2H2O(l)
If 32.59mL NaOH solution is required to reach the endpoint, what
is the molarity of the H2SO4 solution?
1. It requires 10.9 mL of 0.50 M NaOH to neutralize 15.0 mL of
an unknown H3PO4 solution. a. Balance the reaction equation. H3PO4
+ NaOH Na3PO4 + H2O b. Calculate the initial H3PO4 concentration.
2. It requires 28.1 mL of 16.0 mM H2SO4 to neutralize 11.0 mL of an
unknown Ca(OH)2 solution. a. Balance the reaction equation. H2SO4 +
Ca(OH)2 ⇋ CaSO4 + H2O b. Calculate the initial Ca(OH)2
concentration.
50.0 mL of a 0.100 -M HoAc solution is titrated with a 0.100 -M
NaOH solution. Calculate the pH at each of the following
points.
Volume of NaOH added: 0, 5, 10, 25, 40 ,45 , 50 , 55 , 60 , 70 ,
80 , 90 , 100
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!
How many milliliters of 0.100 M NaOH are required to neutralize
the following solutions?
(a) 8.00 mL of 0.0500 M HCL
(b) 20.00 mL of 0.126 M HNO3
(c) 45.00 mL of 0.215 M H2SO4
How many milliliters of 0.100 M HNO3 Are needed to neutralizw
the following solutions
34.7 mL of 0.775 M Naoh _____mL
58.5 mL of 0.0100 M Al(OH)3 ____mL
A 10.0 mL solution of 0.300 M NH3 is titrated with a
0.100 M HCl solution. Calculate the pH after the addition
of 20.0 mL of the HCl solution.
(potentially useful info: Ka of NH4+ = 5.6 x 10−10)