Determine the pH of an HNO2 solution of each of the following
concentrations.
0.540 M
0.100 M
1.30×10−2 M
In which cases can you not make the simplifying assumption that
x is small?
Determine the pH of each solution.
a. 0.155 M HNO2 (for HNO2, Ka=4.6×10^−4)
b. 0.0210 M KOH
c. 0.240 M CH3NH3I (for CH3NH2, Kb=4.4×10^−4)
d. 0.324 M KC6H5O (for HC6H5O, Ka=1.3×10^−10)
Determine the pH of an HF solution of each of
the following concentrations.
Part A: .280 M
PartB : 4.5*10^-2 M
Part C: 2*10^-2
Part D
In which cases can you not make the simplifying assumption that
x is small?
In which cases can you not make the simplifying assumption that
x is small?
only in (a)
only in (b)
in (a) and (b)
in (b) and (c)
Determine the pH of an HF solution of each of the following
concentrations. In which cases can you not make the simplifying
assumption that x is small? (Ka for HF is 6.8×10−4.)
a) 0.260 M
b) 4.80×10−2 M
c) 3.00×10−2 M
Determine the pH of an HNO2 solution of each
concentration. In which cases can you not make the simplifying
assumption that x is small?
a. 0.250 M
b. 0.0500 M
c. 0.0250 M
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]