What is ph when 4.0 ml of 2.0 m barium hydroxide is added to 10.0 ml of 1.00 m nitric acid? 13.63 0.37 0.85 13.15

- pH sis 13.63

Solution:- It is a strong base vs strong acid titration. The equation for the reaction takes place between given acid and base is:

let's calculate the moles of each from given molarities and mL.

moles of barium hydroxide =

= 0.008 mol

moles of nitric acid =

= 0.01 mol

From balanced equation base and acid react in 1:2 mol ratio. So, let's calculate the moles of base used to react with the acid:

=

excess moles of barium hydroxide = 0.008 - 0.005 = 0.003 mol

Total volume of the solution = 0.004L + 0.010 mL = 0.014 L

Concentration of excess barium hydroxide =

= 0.214M

Barium hydroxide as two OH in it. So, the concentration of hydroxide ions will be twice of barium hydroxide concentration.

So,  = 0.428M

pOH = log(0.428)

pOH = 0.37

pH = 14 - pOH

pH = 14 - 0.37

pH = 13.63

First choice is correct, the pH of the solution is 13.63.

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.

може ли да зареждате повече информация, моля