HCl solution, about 250 mL in volume. The pH of the solution is 1.37. Calculate the molar concentration of HCl in this solution. Please use the scientific presentation of the numerical answers (i. e., 1.23x 102), and round your answers to two decimal places.

Molar concentration of HCl in this Solution = 0.01 molar

Explanation:

Given pH = 1.37

So Concentration of H⁺ is equal to = 0.042 molar

Volume of HCl solution = 250 ml

Since,

             1000 ml solution contain 0.042 mole of HCl

              250 ml solution contain = = 0.01 molar

Round off value = 0.01

Molar concentration of HCl in this Solution = 0.01 molar

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.