Estimate the effect of addition of 0.020 mol of NaOH on the pH
of 1.0 dm3...
Estimate the effect of addition of 0.020 mol of NaOH on the pH
of 1.0 dm3 of (a) 0.15 M CH3COONa(aq) and (b)
a buffer solution containing 0.15 M CH3COOH(aq) and 0.15
M NaCH3CO2(aq).
Solutions
Expert Solution
After
adding 0.020mol of NaOH to this weak acid,the pH of the solution
further increases.Since NaOH (aq) reacts with acetic acid.
Calculate the pH of 1.0 L upon addition of 0.190 mol of solid
NaOH to the original buffer solution. Express the pH to two decimal
places. Consider a buffer solution that is 0.50 M in NH3
and 0.20 M in NH4Cl. For ammonia, pKb=4.75.
What is the pH of the solution after the additional of 0.020 mol
of solid NaOH to a 250.0 mL of buffer made of 0.400 M of HF and
0.800 M of KF assuming solution volume does not change
(Ka=7.2 x 10−4)?
1) Calculate the pH of 1.0 L of the solution upon addition of
0.010 mol of solid NaOH to the original buffer solution.
2) Calculate the pH of 1.0 L of the solution upon addition of
30.0 mL of 1.0 MHCl to the original buffer solution.
3) A 1.0L buffer solution contains 0.100 molHC2H3O2 and 0.100
molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.
3A) Calculate the pH of the solution upon the addition of 0.015
mol of NaOH...
A hypothetical weak acid, HA, was combined with NaOH in the following proportions: 0.20 mol of HA, 0.080 mol of NaOH. The mixture was diluted to a total volume of 1.0 L and the pH measured.(a) If pH = 4.80, what is the pKa of the acid?(b) How many additional moles of NaOH should be added to the solution to increase the pH to 5.00?
A.) Calculate the pH of 1.0 L of the solution, upon addition of
49.00 mL of 1.0 MHCl.
Calculate the pH of the solution upon addition of 19.1 mL of
1.00 MHCl to the original buffer
B.)For each of the following solutions, calculate the initial pH
and the final pH after adding 0.005 mol of NaOH.
1.) 300.0 mL of pure water
2.)300.0 mL of a buffer solution that is 0.210 M in HCHO2 and
0.290 M in KCHO2
3.)300.0...
calculate the initial pH and the pH after each 2ml addition of
0.10M NaOH.
i) initial pH
a) 2ml of 0.10M of NaOH has added to 50ml of 0.50M
HC2H3O2/0.050M NaC2H3O2
b) 8ml of 0.10M of NaOH has added to 50ml of 0.50M
HC2H3O2/0.050M NaC2H3O2
c) 10ml of 0.10M of NaOH has added to 50ml of 0.50M
HC2H3O2/0.050M NaC2H3O2
50.0ml of 0.125M HF is titrated with 0.100M NaOH. Calculate the
pH after the addition of
a) 0.00ml of NaOH
b) 15.00ml of NaOH
c) 31.25ml of NaOH
d) 60.00ml of NaOH
e) 62.50ml of NaOH
f) 70.00ml of NaOH
What is the pH after the addition of 20.0 mL of 0.10 M NaOH to
80.0 mL of a buffer solution that is 0.25 M in NH3 and 0.25 M in
NH4Cl, (K b =1.8 x 10 −5 for NH3 )?
Use the data below for O2 gas at 273.15 K:
P (atm)
Vm
(dm3/mol)
(g/dm3)
0.750000
29.8649
1.07144
0.500000
44.8090
0.714110
0.250000
89.6384
0.356975
a. Under what pressure conditions will O2 act most
like an ideal gas and obey the ideal gas law?
b. Rearrange the ideal gas law to solve for the gas law
constant, R.
A 1.0 mol sample of helium gas and a 1.0 mol sample of ammonia
gas are held at the same temperature. Assuming both behave as
ideal gases, do they have the same total internal
energy?