12. Consider the titration of 40.0 mL of 0.500 M NH3 with 1.00 M
HCl a) What is the initial pH of the NH3(aq)? b) What is the pH
halfway to the equivalence point? c) What is the volume of HCl
needed to reach the equivalence point? d) What is the pH at the
equivalence point? e) Sketch the titration curve. Label the
point(s) where there is a A) a weak base B) weak acid C) Buffer D)
Strong acid...
What mass of HCl gas must be added to 1.00 L of a buffer
solution that contains [aceticacid]=2.0M and [acetate]=1.0M in
order to produce a solution with pH = 3.73?
What is the pH of a 1.00 L buffer solution that is 0.80 mol
L-1 NH3 and 1.00 mol L-1
NH4Cl after the addition of 0.070 mol of NaOH(s)?
Kb(NH3) = 1.76 ? 10?5
Calculate the pH after 0.017 mole of HCl is added to 1.00 L of
each of the four solutions. (Assume that all solutions are at
25°C.) (a) 0.128 M butanoic acid (HC4H7O2, Ka = 1.5 ✕ 10−5) (b)
0.128 M sodium butanoate (NaC4H7O2) (c) pure H2O (d) 0.128 M
HC4H7O2 and 0.128 M NaC4H7O2
50.0 mL of 1.00 M of a solution of HCl at 18.0 ºC is
combined with 50.0 mL of 1.00 M solution of NaOH at 18.0 ºC. The
final temperature of the reaction mixture is 24.6 ºC. If the heat
capacities and densities of these solutions are approximately the
same as water (4.184 J/g · ºC, 1.00 g/mL), what is the molar heat
of neutralization (∆Hneut.)? Is this reaction endothermic or
exothermic? [2 pt.]
HCl (aq) + NaOH (aq) →...
What is the pH of a solution made by mixing 500 mL of 1.00 M HCN
and 1.50 L of 0.250 M NaOH, and then diluting the entire solution
to a volume of 3.00 L? (Ka HCN = 4.0 x 10-10)
A.
8.92
B. 6.52
C.
9.88
D.
9.27
E.
5.08
To obtain one litre of a solution of pH = 7, you should dissolve
in water
A.
Two mol of HI + two mol of CH3NH2
B.
One mol...
Calculate the pH of 1.00 L of a solution that is 0.120M in
HNO2 and 0.150M in NaNO2 before and after you
add 2.0mL of 15.0M HCL. [Ka(HNO2) = 4.0 x
10-4]