What is the pH of a solution in which 222 mL of HCl(g), measured at 26.0 ∘C and 1.06 atm, is dissolved in water to give 1.5 L of aqueous solution? (Hint: Use the ideal gas law to find moles of HCl first.)

6.39 × 10⁻³ M

Explanation:

First, we will calculate the moles of HCl using the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.06 atm × 0.222 L / 0.0821 atm.L/mol.K × (26.0 + 273.15) K

n = 9.58 × 10⁻³ mol

The molar concentration of HCl is:

M = moles of HCl / liters of solution

M = 9.58 × 10⁻³ mol / 1.5 L

M = 6.39 × 10⁻³ M

your mom.com . : 0000

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2