calculate the molarity of sodium ion in a solution made by mixing 3.4mL of .386 M soldium chloride with 475mL?

Question

Calculate the molarity of sodium ions in a solution created by mixing 3.4 mL of 0.386 M sodium chloride with 475 mL of 0.0712 M sodium sulfate. Assume the volumes are additive.

Anonymous · Accepted Answer

Determine the total number of moles of Na+ you add

Then determine the conc of this many moles in the total volume

moles = molarity x Litres

moles NaCl = 0.386 M x 0.0034 L

moles NaCl = 0.0013124 moles

Each NaCl has 1 Na+

Therefore moles Na+ from NaCl = 0.0013124 moles

moles Na2SO4 = 0.0712 M x 0.475 L

moles Na2SO4 = 0.03382 moles

Each Na2So4 has 2 Na+

Therefore moles Na+ from Na2SO4 = 2 x 0.03382 = 0.06764 moles Na+

Total moles Na+ = 0.06764 + 0.0013124 = 0.0689524 moles Na+

Total volume = 475 ml + 3.4 ml = 478.4 ml = 0.4784 L

molarity Na+ = moles / L

= 0.0689524 mol / 0.4784 L

= 0.14 M (2 sig figs)

Anonymous · Answer

Your very final concentration of Na+ is a million.496 x 10-2 molar. that’s the way you hit upon it out: Your first answer is 0.280 mole Na+/one hundred mL x 3.68 mL = a million.03 x 10-3 mole Na+ Your 2nd answer is 6.51 x 10-3 mol Na+/one thousand mL x 500 mL X 2 Na+/Na2SO4 formulation unit = 6.51 x 10-3 moles Na+. consisting of them on an identical time provides you 7.fifty 4 x 10-3 moles Na+/0.50368 L, which equals a million.496 x 10-2 moles Na+ in step with liter or a million.496 x 10-2 molar in Na+.

Anonymous

calculate the molarity of sodium ion in a solution made by mixing 3.4mL of .386 M soldium chloride with 475mL?

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