Question

You have an unknown solution of HNO3 and a solution of 0.50 M KOH.
You placed 20 mL of HNO3 into the flask and used 40 mL of KOH from the buret to complete the titration.
8. Write the balanced chemical equation for the acid-base titration.

Answer 1

@ghuczek could you help?

Answer 2

This is an acid-base neutralization ... \[\text{HNO}_{3(aq)} + \text{KOH}_{(aq)} \to \text{H}_2\text{O}_{(l)} + \text{KNO}_{3(aq)} \]

Answer 3

so would it be 20+.50-h20+kno?

Answer 4

The question was to write the balanced equation. That is done. Now think about what you are you trying to find next.

Answer 5

What is the molar ratio of your acid to your base? How did you know?

Answer 6

The balanced equation gives you that. The coefficients for the reactants will give you the mole ratio. What is it?

Answer 7

3 over 0?

Answer 8

1 : 1 ratio in this case.

Answer 9

calculate the concentration of your unknown solution. You MUST show all work to receive full credit

Answer 10

Figure out how many moles of KOH you have. For neutralization you will need an equal number of moles of the acid (because of the 1:1 ratio).
Be careful when finding the final concentration -- assume the volumes of the two solutions are additive once mixed. Good luck.

Answer 11

i really have no idea how

Answer 12

@ghuczek

Answer 13

The first thing to do is find the number of moles of KOH you have.\[\text{number of moles} = \text{molar concentration} \times \text{volume in litres}\]

Answer 14

. 50=not sure what concentration is*not sure either