What are the final hydrogen ion concentration and pH of a solution obtained by mixing 400mL of 0.2M NaOH with 150mL of 0.1M H3PO4?

Answer : The final hydrogen ion concentration is

Explanation :

The chemical reaction equation will be:

In this reaction, 1 mole of reacts with 3 mole NaOH.

So, the number of moles of present in 150 ml of 0.1 M solution is calculated as follows.

Number of moles = Concentration × Volume

Number of moles = 0.1 M ×0.150 L = 0.015 mol

As it reacts with 3 moles of NaOH.

Number of moles of NaOH = 3 × 0.015 mol = 0.045 mol

So, moles of NaOH in 400 mL of 0.2 M NaOH is as follows.

Number of moles =  0.2 M × 0.4 L = 0.080 mol

Number of moles remained after the reaction = (0.080 - 0.045) mol  = 0.035 mol NaOH in 550 ml (400 ml + 150 ml)

As molarity is the number of moles present in liter of solution. Hence, molarity of NaOH is as follows.

Now we have to determine the hydroxide ion concentration.

As, = 0.0636 M

Now we have to determine the pH.

As,  pH + pOH = 14

pH = 14 - pOH

pH = 14 - 1.20

pH = 12.8

Now we have to determine the hydrogen ion concentration.

Therefore, the final hydrogen ion concentration is

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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.