I have the percentage uncertainty of a 0.15 M solution, but I don't know how to calculate the uncertainty for the 0.12, 0.09, 0.06 and 0.03 solutions, can someone help me?

Na2S2O3 Solution:

A 0.15 mol/dm3 solution of sodium thiosulfate was made by finding the mass amount of solid sodium thiosulfate needed to produce the solution using this formula

C = nv

C = Concentration (mol/L)

n = Mols

v = Volume (L)

0.15 = n1

n = 0.151

n = 0.15

Through this formula, it was found that 0.15 mols of sodium thiosulfate was needed. To find this amount in grams, this equation was used.

n = mMM

n = Mols

m = Mass (g)

MM = Molar mass (g/mol)

Molar mass of Sodium Thiosulfate, Na2S2O3 =(22.992) + (32.07 2) + (16.00 3)

= 158.12 g

0.15 = m158.12

m = 0.15158.12

m =23.718 g

23.718 g of sodium thiosulfate was measured on a scale then added to 1 L volumetric flask with water to make the 0.15 mol/L solution

1000 cm3 0.15 M Sodium Thiosulfate solution;

%uncertainty mass = 0.0123.718100 = 0.04216%

%uncertainty volume = 0.51000100= 0.05%

Total uncertainty =0.04216 +0.05 = 0.09216%