Question

A
saturated sodium carbonate solution at 100 degrees celsius contains
45.5 g of dissolved sodium carbonate per 100. mL of solution. The
solubility product constant for sodium carbonate at this temp is

79.0

0.316

0.0790

36.8

316.

Answer #1

Molar mass of Na2CO3 = 2*MM(Na) + 1*MM(C) + 3*MM(O)

= 2*22.99 + 1*12.01 + 3*16.0

= 105.99 g/mol

Molar mass of Na2CO3= 105.99 g/mol

s = 45.5 g/100 mL = 455 g/L = 4.55*10^2 g/L

To covert it to mol/L, divide it by molar mass

s = 4.55*10^2 g/L / 105.99 g/mol

s = 4.293 g/mol

The salt dissolves as:

Na2CO3 <----> Na+ + 2 CO32-

s 2s

Ksp = [Na+][CO32-]^2

Ksp = (s)*(2s)^2

Ksp = 4(s)^3

Ksp = 4(4.293)^3

Ksp = 316

Answer: 316

Sodium carbonate (2.4134 g) is dissolved in enough deionized
water to give a solution with a total volume of 250.0 mL. What is
the pH of the resulting solution? For carbonic acid, pKa1 = 6.351
and pKa2 = 10.329.
Also:
What is the equilibrium concentration of H2CO3 in the
solution
calculate the value of aHCO3โ.
Write a mass balance and charge balance equation
please show all work!

if the solubility of ZnCO3 in water at 25 degrees celsius is
1.54*10^-3 g/L, calculate the solubility-product constant of ZnCO3,
assuming complete dissociaition of ZnCO3 that has dissolved.

Sodium carbonate (2.4134 g) is dissolved in enough deionized
water to give a solution with a total volume of 250.0 mL. What is
the pH of the resulting solution? Hint: For carbonic acid, pKa1 =
6.351 and pKa2 = 10.329. What is the equilibrium concentration of
H2CO3 in the solution? calculate the value of alpha HCO3-. I
already have the answer to the first part of the question. I just
need the equilibrium concentration and value of alpha please!

used Mg for these trials
Trial
HCl (mL)
Mass (g)
Ti degrees Celsius
Tf degrees Celsius
#1
7.5 mL
0.08 g
24 o C
62.0 o C
#2
7.5 mL
0.05 g
24.9 o C
57.9 o C
used MgO for these trials
Trial
HCl (mL)
Mass (g)
Ti degrees Celsius
Ti degrees Celsius
#1
7.5 mL
0.13 g
23.3 o C
30.1 o C
#2
7.5 mL
0.15 g
22.7 o C
36.8 o C
Ti = initial temperature...

A solution is prepared by dissolving 11.3 g of a mixture of
sodium carbonate and sodium bicarbonate in 1.00 L of water. A 300.0
cm3 sample of the solution is then treated with excess HNO3 and
boiled to remove all the dissolved gas. A total of 0.940 L of dry
CO2 is collected at 298 K and 0.972 atm. Find the molarity of the
carbonate in the solution and the molarity of the bicarbonate in
the solution.

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cm3 sample of the solution is then treated with excess HNO3 and
boiled to remove all the dissolved gas. A total of 0.940 L of dry
CO2 is collected at 298 K and 0.972 atm.
1.Find the molarity of the carbonate in the solution.
2.Find the molarity of the bicarbonate in the solution.

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