Question

Calculate the PH of 1 mole of 1m Hcl solution diluted to 1 litre
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Answer 1

Answer:

Let us suppose that you have available 37 wt% hydrochloric acid of some commercial brand (reagent grade). Unless stated otherwise, the concentration indicated in the label, should be assumed as given in wt%. The corresponding (approx.) density should be available from the label, but we can also take it as 1.184 g·cm-3 (cf. e.g. Perry's Chemical Engineers' Handbook). The molecular mass of HCl is 36.46 g·mol−1. From this data the molarity of the conc. sol. is readily calculated. The intended dilute solution (1 M) should be prepared by considering the appropriate (volumetric) dilution factor.

Explanation:

OR

Commercial concentrated HCl:

Specific gravity = 1.19

1.19g of HCl in 1ml of water

Assay= 37.4%

37.4ml of HCl in 100ml of water

i.e. 37.4 x 1.19 = 44.506g of HCl in 100ml of water

Commercial concentrated HCl:

Specific gravity = 1.19

1.19g of HCl in 1ml of water

Assay= 37.4%

37.4ml of HCl in 100ml of water

i.e. 37.4 x 1.19 = 44.506g of HCl in 100ml of water

Formula weight = 36.46

1M = 36.46 g HCl in 1000ml of water

So if 44.506g of HCl is present in 100ml of water

Or 445.06g of HCl is present in 1000ml of water

Molarity of that solution is 445.06 / 36.46 = 12.2

Thus molarity of concentrated HCl is 12.2 M

Formula weight = 36.46

1M = 36.46 g HCl in 1000ml of water

So if 44.506g of HCl is present in 100ml of water

Or 445.06g of HCl is present in 1000ml of water

Molarity of that solution is 445.06 / 36.46 = 12.2

Thus molarity of concentrated HCl is 12.2 M