Calculate the molarity of a 10.0% (by mass) aqueous solution of hydrochloric acid. the density of this solution is 1.01 g/ml. a. 0.277 m b. 2.77 m c. 3.04 m d. 4.33 m e. the density of the solution is needed to solve the problem

[HCl] = 2.77 M   (option b)

Explanation:

A 10% by mass is an information that means, 10 g of solute are contained in 100 g of solution.

Density is mass / volume and it always corresponds to solution.

So solution mass is 100 g. Let's find out solution volume with density

Solution mass / Solution volume = Solution density

100 g / Solution volume = 1.01 g/mL

100 g / 1.01 g/mL = 99 mL

In conclusion our 10 g of HCl are contained in 99 mL of solution

Molarity is mol of solute in 1L of solution

Let's convert the mass to moles (mass / molar mass)

10 g / 36.45 g/mol = 0.274 moles

Let's convert the mL in L

99 mL = 0.099L

Molarity is mol/L → 0.274 mol / 0.099L = 2.77M

43.452

step-by-step explanation:

284 times .153 = 43.452

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.