8.00 ml of nh3 is titrated directly from 32.6 ml of 0.4000 m hcl what is the concentration of the nh3 in the solution

1.63 M

The reaction between NH₃ and HCl is given by the equation;

NH₃(aq) + HCl(aq) → NH₄Cl(aq)

We want to calculate the concentration of ammonia solution.

Step 1: Calculate the number of moles of HCl used

To calculate the number of moles we multiply the molarity of HCl by the volume.

Moles = Molarity × Volume

          = 0.40 M × 0.0326 L

          = 0.01304 moles

Step 2: Determine the number of moles of NH₃

From the equation 1 mole of HCl reacts 1 mole of NH₃

Therefore, the mole ratio of HCl to NH₃ id 1 : 1

Hence, the number of moles of HCl are equal to the number of moles of NH₃

Number of moles of NH₃ = 0.01304 moles

Step 3: Calculate the concentration of NH₃

Molarity is the concentration of a solution in moles per liter

Molarity = Number of moles ÷ Volume

Number of moles = 0.01304 moles

Volume of NH₃ =8.00 mL or 0.008 L

Therefore;

Molarity = 0.01304 moles ÷ 0.008 L

            = 1.63 M

Therefore, the concentration of NH₃ IS 1.63 M

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.