Question

Commercially available concentrated Hcl contains 38% Hcl by mass. (1) what is the molarity of the solution ( density of solution =1.19 g mL -1)

(2) What volume of concentrated Hcl is required is required to make 1.0 L of an 0.10 M Hcl.

Answer 1

Molarity= 12.61 Molar and 7.96ml of HCl (38%) needed for 1.0 liter of 0.10. Molar HCl (aq)
Explanation of questions 1)
HCl (38%)=(38q/100soln)=(? moles HCl/1.0 liter solution)
=>Moles of HCl in 38 grams= (38gHcl/36(g/mol) = 1.06 mole HCl
=>volume of solution (liters) containing 1.06 mole if HCl =100g HCl (38%)/1.19(g/ml)=0.084L HCl (38%)
=>Molarity HCl (38%)= 1.06 mole HCl/0.084L HCl Conc=12.62 Molar HCl (aq)
question 2)
use the solution prep equations of liquid mfg Stock.
volume of liquid Mfg Stock need de in mil liters
=>vol of mfg=(Molarity) (Volume= (formula Weight)/(Purity) (Specific Gravity)
=>(0.10M) (1.0L) (36(g/mole))/(0.38) (1.9(g/ml) = 7.96 mol HCl (38%)
Mixing:- Add 7.96 ml of HCl (38%) into a small quantity of water, mix to disperse; then dilute with solvent water hoti but not exceed the total needed volume of solution (in the case 1.00 Liter)
=> Solution:- Verify concentration with standardized NaOH (solution).
Mixing Caution:- Always add a concentrated of water; hoti,but not to exceed needed total volume solution.
water onto bulk strong concentrated acid may result in uncountable heat generation and flash boiling due to accelerated ionization rate
Certainly wear protective eye ware and appropriate clothing.

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