A chemist dissolves of pure nitric acid in enough water to make up of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

The given question is incomplete. The complete question is

A chemist dissolves 314 mg of pure nitric acid in enough water to make up 190 ml of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

where,

n= moles of solute=

= volume of solution in ml = 190 ml

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

1 mole of gives 1 mole of

Thus 0.026 moles of give= of

Putting in the values:

Thus pH of the solution is 1.58

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.