A typical dose of FeSO_4 is 0.46 g. How many milliliters of a 0.26 M FeSO_4 solu

Question

A typical dose of FeSO_4 is 0.46 g. How many milliliters of a 0.26 M FeSO_4 solution is needed to supply this dose? A nurse needs to prepare a 1.0% (m/v) solution of silver nitrate from 62 mL of a 4.0 % (m/v) stock solution. How much water should be added to the 62 mL of stock solution? How many grams of sucrose should be added to 535 g of water to produce a solution that is 0.925% (m/m) sucrose? What is the osmolarity of a 0.0815 M solution of ammonium phosphate? Which of the following statements about solutions is incorrect? The solubility rule "like dissolves like" is not adequate for predicting solubilities when the solute is a(n) In which of the following pairs of properties are both members of the pair colligative properties? Addition of a nonvolatile solute to a solvent produces a solution with a lower vapor pressure, a lower freezing point, and a higher boiling point than that of a pure solvent. Osmotic pressure is the amount of pressure needed to prevent the process of osmosis from occurring.

Explanation / Answer

60) We know the formula for molarity that is

M = (weight / molecular weight) x (1000 / Volume)

weight = 0.46 g,

FeSO4 molecular weight = 151.908 g/mole

Molarity M = 0.26

Volume = ?

Plug all the values in the above equation, then we will get

V = (weight / molecular weight) x (1000 / Molarity) = 11.647 ml

61)

In such case we have to use dilution law i.e M1V1 = M2V2

M1 = 4.0 % m/v , V1 = 62 ml

M2 = 1.0 % , V2 = ?

V2 = M1 x V1 / M2 = 248 ml

62)

Let us assume weight of sucrose = w

% m/m sucrose = mass of sucrose / total mass x 100

0.925 / 100 = (w / w+535)

if solved we will get weight = 4.995 g

64) Ans: C

65) Ans: D, because ionic campouns can be polar or non polar

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