a) A beaker contains 200.0 mL of 0.250 M AgNO3. 200.0 mL of
0.100 M HCl(aq) is added to it. What is the NO3− concentration in
the final mixture?b) What is the Ag+(aq) concentration in the final
mixture? (Hint: does anything happen when you mix these
solutions?)
What is the concentration of hydroxide ions after 50.0 mL of
0.250 M NaOH is added to 120 mL of 0.200 M Na2SO4?
What is the concentration of hydroxide ions after 50.0 mL of
0.250 M NaOH is added to 120 mL of 0.200 M Sr(OH)2?
Consider the following four titrations.
i. 100.0 mL of 0.10 M HCl titrated by 0.10 M
NaOH
ii. 100.0 mL of 0.10 M NaOH titrated by 0.10 M
HCl iii. 100.0 mL of 0.10 M CH3NH2 titrated by 0.10
M HCl
iv. 100.0 mL of 0.10 M HF titrated by 0.10 M
NaOH Rank the titrations in order of:
increasing volume of titrant added to reach the equiva-
lence point.
increasing pH initially before any titrant has been added.
increasing...
Assume 200. mL of 0.400 M HCl is mixed with 200 mL of 0.250 M
Ba(OH)2 in a constant-pressure calorimeter. The temperature of the
solutions before mixing was 25.10C; after mixng and alowing the
reaction to occur, the temperature is 27.78C.
Determine ΔrH for this reaction in units of
kJ/mol-rxn.
2 HCl(aq) + Ba(OH)2(aq) -> BaCl2(aq) + 2 H2O(l)
The densities of all solutions are 1.00 g/mL
The specific heat capacitites of all solutions are 4.20 J/(gC)
2)
A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M
HCl.
Determine the following quantities:
a)
The initial pH of the KOH solution before any acid is added.
b)
The pH of the solution after 3.00 mL of HCl is added.
c)
The quantity of HCl solution required to reach the
equivalence
point.
d)
The pH of the solution at the equivalence point.
e)
The pH of the solution after20.0 mL of HCl is added.
Draw titration curve if titrate 10.00 mL of 0.250 M
CH3NH2 with 0.125 M HCl. Also, calculaute pH@ 0.0 mL, 5.00 mL,
10.00 mL, 20.00 mL, 20.50 mL
Please explain everything you are doing so I could
understand how you solved. Do not write in cursive.
Draw titration curve if titrate 10.00 mL of 0.250 M
CH3NH2 with 0.125 M HCl. Also, calculaute pH@ 0.0 mL, 5.00 mL,
10.00 mL, 20.00 mL, 20.50 mL
Please explain everything you are doing so I could
understand how you solved. Do not write in cursive.
a. What volume of 0.085 M HCl is required to titrate 25.00 mL of
a 0.100 M NH3 solution to the equivalence point?
b. What is the pH at the equivalence point?
What volume of 0.496 M HCl is required to neutralize 20.0 mL of
0.809 M sodium hydroxide? b.) If you added 35.0 mL of hydrochloric
acid solution to the sodium hydroxide, will the resulting solution
be acidic or basic? Explain your reasoning. c.) Describe how you
would neutralize the new solution using amounts (in volume) of
either 0.496 M HCl or 0.809 M sodium hydroxide.