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It is 11.3

Q: What is the molarity of 35 per cent Hydrochloric acid solution with specific gravity of 1.8 gram per liter?

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1.12

It depends on the concentration.

1.3

It depends on the solution's degree of concentration or dilution.

Electrolyte of sulphuric acid to a specific gravity of 1250.

Related questions

The specific gravity of pure water is 1.0000 at 4 °C and 1 bar. Deviations from this will change the specific gravity. At 0°C and 1 bar, liquid water has a specific gravity of 0.9999 (one of the only substances to EXPAND as it approaches its freezing point). At 100 °C and 1 bar, the specific gravity of liquid water is 0.9584. At 0 °C and 150 bar, liquid water has a specific gravity of about 1.007.

1.12

It depends on the concentration.

Molarity =(% by weight x density x 1000 mL/litre)/(Molecular weight x 100%) %by weight ={(Molarity x Molecular Weight)/(density x 1000 mL/litre)} x 100% Molecular weight - grams/mol (36.461 g/mol for HCl) Molarity - mol/litre Density - g/millilitre (Density may be listed as specific gravity) For the given conditions Conc.HCl 37.0%, sp.gr. 1.19 Molarity = (37.0 x 1.19 x 1000)/(36.461 x 100) Molarity = 12.07592 M Available = 12.07592 M HCl Required = 0.300 M HCl: V1 x C1 = V2 x C2 (1000[mL] x 0.300[M]) / (12.07592[M]) = 24.84283[mL] Dilute 24.84mL of 37.0% HCl to one liter to get 0.300M HCl solution.

1.3

489 grams

It depends on the solution's degree of concentration or dilution.

Electrolyte of sulphuric acid to a specific gravity of 1250.

answer lies within "specific gravity".

335.7*1.06 = 355.842 grammes

To find the molarity, we can set up the following factor labeling problem. Note that a specific gravity of 1.84 can be treated as a density of 1.84 g/ml. The molar mass of sulfuric acid (H2SO4) is 98.079 g /molM(mol/l)= (1.84 g/ 1 ml)(1000 ml/1 l)(1 mol/98.079 g)(.96 purity)= 18 mol/l= 18 MThe molarity is 18 mol/l. The pH of this solution would be -1.26...VERY ACIDIC.

The density (the expression specific gravity is obsolete) of NaCl is2,165 g/cm3.