How many grams of #CuSO_4# are present in 652 mL of .250 M #CuSO_4# solution?
2 Answers
Approx.
Explanation:
We use the defining quotient....
And thus
And for
And with respect to
Of course in an aqueous solution of copper sulfate, the copper is present as
Explanation:
Given the molarity
#M=eta/V# where:
#eta=("mass"(m))/("molar mass"(Mm))#
Now, plug in this value to the formula. Rearrange formula to isolate
#M=((m)/(Mm))/V# ; cross multiply to simplify
#MV=m/(Mm# ; isolate the required variable#m#
#m=MVMm# ; now, plug in the values of each variablewhere:
#M=0.250M=(0.250mol)/(L)#
#V=652cancel(mL)xx(1L)/(1000cancel(mL))=0.652L#
#Mm_(CuSO_4)=(159.5g)/(mol)# , obtainable from the periodic table.
#m=(0.250cancel(mol))/cancel(L)xx0.652cancel(L)xx(159.5g)/cancel(mol)#
#m=ul ?g CuSO_4#