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

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

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