50.0 mL of 10.0 M sodium hydroxide is added to a 1.00 L solution
containing 0.100...
50.0 mL of 10.0 M sodium hydroxide is added to a 1.00 L solution
containing 0.100 M nickel (II) nitrate, 0.100 M tin (II) nitrate,
and 0.100 M zinc nitrate. How many grams of tin (II) hydroxide
precipitates from solution.
Solutions
Expert Solution
I have given the answer in three significant figures.....if the
answer does not match due to significant figures then please
comment below.....
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of
1.00 M NaCl solution at 25.0 ° C in a calorimeter, a white
precipitate of AgCl forms and the temperature of the aqueous
mixture increases to 32.6 ° C. Assuming that the specific heat of
the aqueous mixture is 4.18 J/(g °C), the density of the mixture is
1.00 g/mL, and the calorimeter itself absorbs a negligible amount
of heat, what is ΔH in kJ/mol AgCl...
For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M
sodium hydroxide, determine the pH when:
(a) 50.0 mL of base has been added.
(b) 75.0 mL of base has been added.
(c) 100.0 mL of base has been added.
A student reaceted 50.0 ml of 1.05 N sodium hydroxide with 50.0
ml of 1.00 N sulfuric acid in a coffee cup calorimeter. From the
temperature vs time plot, the average Ti was 25.7 celsius and the
Tf of the reaction mixture was 31.2 Celsius. (ignore calorimeter
constant).
What is the enthalpy of neutralization?
A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of
0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the
resulting solution. The Ksp value for AgIO3(s) is 3.17 × 10-8.
[Ag+] =____ mol/L
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
50.0 mL of 2.00 mol/L HNO3 solution and 50.0 mL of 1.00 mol/L
NaOH solution, both at 20.0 degree Celsius, were mixed in a
calorimeter. Calculate the molar heat of neutralization of HNO3 in
kJ/mol if:
(1) final temperature was 28.9 degree Celsius;
(2) the mass of the overall solution was 102.0 g;
(3) the heat capacity of the calorimeter was 25.0 J/C;
(4) and assume that the specific heat of solution is the same as
water, 4.184 J/(g C);
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of
0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5.
a. Calculate the pH of both solutions before mixing.
b. Construct an ICE table representative of this mixture.
c. Determine the approximate pH of the solution.
d. Determine the percent ionization of the acetic acid in this
mixture
20.0 mL of 0.100 M copper(II) sulfate reacts with 20.0 mL of
0.100 M sodium hydroxide to form a precipitate (Cu(OH) 2 2 ). What
is the concentration (molarity) of Cu 2+ in the resulting
solution?