Question
In: Chemistry
Equal volumes of a 0.020 M Zn^2+ solution and a 2.0 M NH3 solution are mixed....
Equal volumes of a 0.020 M Zn^2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3)4]^2+ is 4.1 × 10^8. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10^-8
Answer: no, Q = 2.9 × 10^-12
Solutions
queen_honey_blossom answered 3 years agoRelated Solutions
Equal volumes of 0.180 M AgNO3 and 0.160 M ZnCl2 solution are mixed. Calculate the equilibrium...
Equal volumes of 0.180 M
AgNO3 and 0.160
M ZnCl2 solution are
mixed. Calculate the equilibrium concentrations of
Ag+ and
Zn2+.
Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M...
Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with
a 0.020 M solution of hydrochloric acid. A) Write the chemical
equation that occurs B) Do you expect the pH of the solution to be
acidic, basic or neutral at the equivalence point? Explain. C)
Calculate the pH after 20 mL of HCl solution have been added. Hint:
Kb(NH3)=1.8*10-5
A solution is made that is 1.1×10−3 M in Zn(NO3)2 and 0.140 M in NH3. Part...
A solution is made that is 1.1×10−3 M in Zn(NO3)2 and 0.140 M in
NH3.
Part A
After the solution reaches equilibrium, what concentration of
Zn2+(aq) remains?
Express your answer using two significant figures.
A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is slowly mixed with...
A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is
slowly mixed with 0.100 M HCl. Determine the pH after addition
of:
0 mL of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, 250 mL
of HCl
4. Describe in exact detail (including gram quantities and
identity of species) how you would create a 500 mL solution of
buffer with a pH 8.0 ?
A solution is made of 1.1 x 10-3M in Zn(NO3)2 and 0.150 M in NH3. After...
A solution is made of 1.1 x
10-3M in
Zn(NO3)2 and 0.150 M
in NH3.
After the solution reaches equilibrium, what
concentration of Zn2+(aq) remains?
Kf (Zn(NH3)42+) = 2.8 x
109
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly
mixed with .100 M HCl. Determine the pH after addition of: 0 ml of
HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of
HCl.
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly
mixed with .100 M HCl. Determine the pH after addition of: 0 ml of
HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of
HCl.
PART A) A solution is prepared by mixing equal volumes of 0.17 M HCl and 0.42...
PART A)
A solution is prepared by mixing equal volumes of 0.17 M HCl and
0.42 M HNO3. (Assume that volumes are additive.) Express the pH to
two decimal places.
PART B)
Using the chart Estimate [H3O+] in a 1.5 M solution of
each acid.
Express the molar concentrations to two significant figures
separated by commas.
I'm stuck on the one that says very
large. For all the other ones I multiplied the Ka by
the 1.5M. The answer for...
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M...
A buffer solution is prepared from equal volumes of 0.200 M
acetic acid and 0.600 M sodium acetate use 1.80 *10^-5 as Ka for
acetic acid.
a.) what is the pH of the solution
b.) Is the solution acidic or basic
c.) What is the pH of a solution that results when 3.00ml of
0.034 M HCl is added to 0.200L of the original buffer
Question 6 Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M...
Question 6
Calculate the pH of a solution prepared by mixing equal volumes
of 0.050 M sodium oxalate, Na2C2O4 (aq), and 0.010 M
ammonium chloride, NH4Cl (aq).
For ammonium, Ka = 5.70 × 10–10; for oxalic acid,
Ka,1 = 5.60 × 10–2and Ka,2 = 5.42 × 10–5.
Hint #1: Use the charge balance
equation as your main equation. Use the mass balance and
equilibrium equations to find an expression for each species in
terms of [H3O+] or [OH–], then substitute...
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