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A sample of 0.0084 mol of HCl is dissolved in water to make a 1500 mL solution. Calculate the molarity of the HCl solution, the [H3O+] and the pH. For a strong acid such as HCl, the [H3O+] is the same as the molarity of the HCl solution.
A sample of 0.0084 mol of HCl is dissolved in water to make a 1500 mL solution. Calculate the molarity of the HCl solution, the [H3O+] and the pH. For a strong acid such as HCl, the [H3O+] is the same as the molarity of the HCl solution.
A solution prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution has aMolarityofHClof5.6 × 10⁻³ M, aMolarityofH₃O⁺of5.6 × 10⁻³ Mand apHof2.3.What is Molarity ?Molarity (M) is theamountof asubstancein acertain volumeofsolution.Molarity is defined as themolesof asolute per litersof asolution.Molarity isalso knownas themolar concentrationof a solutionA solution is prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution. The molarity of HCl is:[HCl] = 0.0084 moles / 1.5 L=5.6 × 10⁻³ MHClis astrong acidaccording to the following equation.HCl(aq) + H₂O(l) ⇒ Cl⁻(aq) + H₃O⁺(aq)Thus, theconcentrationofH₃O⁺will beequalto theinitialconcentrationof HCl,5.6 × 10⁻³ M.Now, we willcalculatethepHof thesolutionusing itsFormula ;pH = - log[H₃O⁺]= - log [5.6 × 10⁻³]= 2.3Hence, A solution prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution has aMolarityofHClof5.6 × 10⁻³ M, aMolarityofH₃O⁺of5.6 × 10⁻³ Mand apHof2.3.Learn more aboutpHhere ;brainly.com/question/14950262#SPJ1...