you are given a solid that is a mixture of na2s04 and k2s04. A0.215g sample of the mixture is dissolved in water. An excess of an aqueous solution of bacl2 is added. The bas04 that is formed is filtered dried and weight. Its mass is 0.299g what mass of s04 ions is the sample
My calculation 0.299g/233.4g/mol = 0.00128
0.00128 x 96g/mol = 0.123g s04
What is the mass percent of s04 ion in the sample
0.123g/0.215 x 100 = 57.2%
what are the percent composition by mass of na2s04 and k2s04
x/142 = y/174 = 0.00128
Who helps me to solve this part
To solve the part where you need the percent composition by mass of Na2SO4 and K2SO4 in the mixture, you can use a system of equations. Let's assume the mass percent of Na2SO4 is x and the mass percent of K2SO4 is y.
We know that the mass of Na2SO4 in the mixture is equal to (x/100) multiplied by the total mass of the mixture (0.215g), and the mass of K2SO4 is (y/100) multiplied by the total mass of the mixture.
So, we have the equation: (x/100) * 0.215g + (y/100) * 0.215g = 0.00128g (since 0.00128g is the mass of SO4 ions).
Similarly, we can use the molar masses of Na2SO4 (142g/mol) and K2SO4 (174g/mol) to get another equation:
(x/100) * 142g + (y/100) * 174g = 0.00128g
To solve this system of equations, you can use substitution or elimination methods.
Let's use substitution:
From the first equation, we can solve for (x/100):
(x/100) = (0.00128g - (y/100) * 0.215g) / 0.215g
Now, we substitute this value for (x/100) in the second equation and solve for y:
((0.00128g - (y/100) * 0.215g) / 0.215g) * 142g + (y/100) * 174g = 0.00128g
Simplifying and solving for y will give you the mass percent of K2SO4. Then, you can subtract this value from 100 to get the mass percent of Na2SO4.
Since this calculation involves substitutions and simplifications, it may be helpful to use a calculator or online solver tool to obtain the final values of x and y.