Question

In: Chemistry

A 1000.-mL solution of hydrochloric acid has a pH of 1.6. Calculate the mass (g) of...

A 1000.-mL solution of hydrochloric acid has a pH of 1.6. Calculate the mass (g) of HCl dissolved in the solution.

Solutions

Expert Solution

Given pH = 1.6

pH = - log [H+]

[H+] = 10 -pH

        = 10 -1.6

        = 0.025 M

HCl H+ + Cl-

1 mole of HCl produces 1 mole of H+

So [HCl] = [H+] = 0.025M

                       = 0.025 mol/L

Given Volume of the solution is = 1000.0 mL = 1 L

So number of moles of HCl in the solution , n = 0.025 mol

Molar mass of HCl = At.mass of H + At.mass of Cl

                            = 1 + 35.5

                            = 36.5 g/mol

We know that Number of moles , n = mass/molar mass

                  So mass of HCl , m = number of moles x molar mass

                                               = 0.025 mol x 36.5 (g/mol)

                                               = 0.917 g

Therefore the mass of HCl dissolved in the solution is 0.917 g


Related Solutions

How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL)...
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 1.80?
What is the pH for a 400 ml solution of 1.6 M Benzoic Acid? If you...
What is the pH for a 400 ml solution of 1.6 M Benzoic Acid? If you added 75 grams of conjugate base (NaC6H5CO2) to the solution, what would the new pH be? If you now added 75 ml of 1.35 M NaOH, what would be the new pH?
Calculate the molarity of a solution made by adding 25.4 mL of concentrated hydrochloric acid (37.3...
Calculate the molarity of a solution made by adding 25.4 mL of concentrated hydrochloric acid (37.3 % by mass, density 1.19 g/mL) to some water in a volumetric flask, then adding water to the mark to make exactly 500 mL of solution. (It is important to add concentrated acid or base to water, rather than the other way, to minimize splashing and maximize safety.)
A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of...
A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of 1.02 g/mL.   The molality of hydrochloric acid in the solution is ____ m. B) An aqueous solution of iron(III) sulfate has a concentration of 0.192 molal.   The percent by mass of iron(III) sulfate in the solution is ____ %.
A solution consists of 44.3 g of hydrochloric acid (HCl), 75.7 g water, and has a...
A solution consists of 44.3 g of hydrochloric acid (HCl), 75.7 g water, and has a volume of 101 mL. Calculate the weight percent of HCl, the molality of HCl, the mole fraction of HCl, and the molarity of HCl in the solution. weight percent = % molality = m mole fraction = molarity = M A solution of barium chloride (BaCl2) in water is 5.000 % barium chloride by mass. Its density is 1.0434 g cm-3 at 20 °C....
When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum...
When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum metal, how many moles of hydrogen gas would be produced? 6HCl(aq) + 2Al(s) → 2AlCl3(aq) + 3H2(g)
Calculate the molar concentration of the acid if 125 mL of hydrochloric acid was required to...
Calculate the molar concentration of the acid if 125 mL of hydrochloric acid was required to neutralize 45.0 mL of 0.345 M lithium hydroxide. Be sure to use a balanced equation.
Concentrated hydrochloric acid solution is 37.0% HCL and has a density of 1.19g/ml. A dilute solution...
Concentrated hydrochloric acid solution is 37.0% HCL and has a density of 1.19g/ml. A dilute solution of HCL is prepared by diluting 4.50mL of this acid to 100.00mL with water. Then 10.0mL of the dilute HCL is used for the reaction with AgNO3 solution as shown below: HCL(aq)+AgNO3(aq) to HNO3(aq)+AgCL(s) How many mL of 0.1105M AgNO3 solution is required to precipitate all of the chloride as AgCl(s)? Please show how you get the answer. Thank you!
A 12.0 mass % solution of H3PO4 in water has a density of 1.104 g/mL. Calculate...
A 12.0 mass % solution of H3PO4 in water has a density of 1.104 g/mL. Calculate the pH in the solution. Ka1= 7.1 × 10−3 Ka2 = 6.3 × 10−8 Ka2 = 4.2 × 10−13
What is the pH when 30 ml of 1M hydrochloric acid is added to 200 mL...
What is the pH when 30 ml of 1M hydrochloric acid is added to 200 mL of distilled water? please writing hot to solve it .
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT