Question

How many moles of protons are present in 35.0 ml of a 4.70 m solution of nitric acid?

Answer 1

To find out the number of moles of protons in 35.0 ml of a 4.70 M solution of nitric acid, we multiply the molarity (4.70 M) by the volume in liters (0.035 L), resulting in 0.1645 moles of protons, since each HNO3 molecule donates one proton.

Step-by-step explanation:

The question asks us to determine the number of moles of protons present in a 35.0 ml of a 4.70 molar solution of nitric acid (HNO3). First, we need to convert the volume from milliliters to liters. There are 35.0 ml of the solution, which is equivalent to 0.035 liters (because 1 liter is 1000 milliliters). Then, we can calculate the number of moles of HNO3 using the formula:

Number of moles = Molarity × Volume (in liters).

For a 4.70 M solution of HNO3:

Number of moles of HNO3 = 4.70 mol/L × 0.035 L = 0.1645 moles.

Since each molecule of HNO3 contains one proton (in the H+ ion), there are also 0.1645 moles of protons present in 35.0 ml of a 4.70 M solution of HNO3.

Answer 2

0.158 mol H+

Step-by-step explanation:

Trying to find moles of protons in 35mL of a 4.50 M solution of nitric acid (HNO3). HNO3 split up is H+ and NO3-. NO3- is negatively charged and we are trying to find protons, which are positively charged, so you gotta go with H+. Find moles of H+ in HNO3.

Math:

35.0 mL x 1 L/1000 mL = 0.035 L

Find: Mol H+/L

Mol H+/L = (4.50 mol HNO3/1 L) x (0.035 L/1 mol HNO3) x (1 mol H+/1 mole HNO3) = 0.158 mol H+