Question

A mixture of Na2CO3 and NaHCO3 has a mass of 82.6 g . It is dissolved in 1.00 L of water and the pH is found to be 9.92.

Find the mass of NaHCO3 in the mixture.

Express your answer with the appropriate units.

m=

Answer #1

Calculate the pH of a solution by mixing 3.29 g of "bicarb",
NaHCO3, and 4.15 g of NA2CO3 in water to form 4.71 L of solution.
The Ka1 for H2CO3 IS 4.31X10^-7 AND THE KA2 IS 4.40X10^-11.

Calculate the molar mass of NaHCO3(s), Na2CO3(s), and CO2(g)
Calculate the number of moles of HCl contained in the two volumes
of HCl solution (25.0ml and 50.0mL: remember to use the molarity of
the solution rather than the molar mass of HCl to find
molarity).

Calculate the mass of butane needed to produce 82.6 g of carbon
dioxide. Express your answer to three significant figures and
include the appropriate units.

How many grams of Na2CO3 (FM 105.99)
should be mixed with 6.41 g of NaHCO3 (FM 84.01) to
produce a 100 mL of buffer with pH of 10.14? (The
Ka's of carbonic acid are
Ka1 = 4.46 ✕ 10−7 and
Ka2 = 4.69 ✕ 10−11.)
NOTE: Use three significant figures in answer.

A mixture of NaCN and NaHSO4 consists of a total of 0.60 mol.
When the mixture is dissolved in 1.0 L of water and comes to
equilibrium the pH is found to be 9.6.
Find the amount of NaCN in the mixture.

Part A
0.75 g of hydrogen chloride (HCl) is dissolved in water to make
7.0 L of solution. What is the pH of the resulting
hydrochloric acid solution?
Express the pH numerically to two decimal places.
pH =
Part B
0.25 g of sodium hydroxide (NaOH) pellets are dissolved in water
to make 8.0 L of solution. What is the pH of this solution?
Express the pH numerically to two decimal places.
pH =

A 0.3146 g sample of a mixture of NaCl(s) and KBr(s) was
dissolved in water. The resulting solution required 54.50 mL of
0.08765 M AgNO3(aq) to precipitate the Cl−(aq) and Br−(aq) as
AgCl(s) and AgBr(s).
Calculate the mass percentage of NaCl(s) in the mixture.
Mass Percentage:__________________

A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was
dissolved in water. The resulting solution required 39.10 mL of
0.08765 M AgNO3(aq) to precipitate the Cl–(aq) and Br–(aq) as
AgCl(s) and AgBr(s). Calculate the mass percentage of NaCl(s) in
the mixture.
PLEASE explain your thought process. I would like to understand
how to get to the answer. Thank you!

Assuming you weighed out a 2.3684 g
sample of your unknown, and dissolved and diluted it as in the
procedure below, and it took 35.63 mL of a 0.1025 M HCl titrant to
reach the endpoint, what are the weight percents of
Na2CO3 and NaHCO3 in your unknown
sample?
Hints:
-Set g Na2CO3 =
X
-Eqn A: bicarbonate + carbonate = diluted weighted mass
(remember, the mass is not 2.3684, you diluted it
before you titrated it.Calculate the diluted g...

A mixture of C3H8 and C2H2 has a mass of 2.6 g . It is burned in
excess O2 to form a mixture of water and carbon dioxide that
contains 1.6 times as many moles of CO2 as of water.
Find the mass of C2H2 in the original mixture.

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