Suppose you have a bottle of aqueous solution labeled \"53.4(+or- 0.4)% (wt/wt)N

Question

Suppose you have a bottle of aqueous solution labeled "53.4(+or- 0.4)% (wt/wt)NaOH whose density is 1.52(+or- 0.01) g/ml".
A) How many ml of 53.4% NaOH are needed to prepare 2.000 L of 0.169 M NaOH?
B) If the uncertainty in delivering the NaOH is (+or- 0.10 ml), calculate the absolute uncertainty in the molarity (0.169 M). A 2-liter volumetric flask was used in preparing the solution. You may assume negligible uncertainty in the molecular weight of NaOH as long as you use the maximum number of digits available for atomic numbers. Suppose you have a bottle of aqueous solution labeled "53.4(+or- 0.4)% (wt/wt)NaOH whose density is 1.52(+or- 0.01) g/ml".
A) How many ml of 53.4% NaOH are needed to prepare 2.000 L of 0.169 M NaOH?
B) If the uncertainty in delivering the NaOH is (+or- 0.10 ml), calculate the absolute uncertainty in the molarity (0.169 M). A 2-liter volumetric flask was used in preparing the solution. You may assume negligible uncertainty in the molecular weight of NaOH as long as you use the maximum number of digits available for atomic numbers.
A) How many ml of 53.4% NaOH are needed to prepare 2.000 L of 0.169 M NaOH?
B) If the uncertainty in delivering the NaOH is (+or- 0.10 ml), calculate the absolute uncertainty in the molarity (0.169 M). A 2-liter volumetric flask was used in preparing the solution. You may assume negligible uncertainty in the molecular weight of NaOH as long as you use the maximum number of digits available for atomic numbers.

Explanation / Answer

Preparing secondary solutions

M of stock solution = {[53.4(

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