Asolution is prepared by adding 49.3 ml concentrated hydrochloric acid and 19.5 ml concentrated nitric acid to 300 ml water. more water is added until the final volume is 1.00 l. calculate h and the ph for this solution. [hint: concentrated hcl is 38% hcl (by mass) and has a density of 1.19 g/ ml; concentrated hno3 is 70% hno3 (by mass) and has a density of 1.42 g/ml.]
[h+] =
oh- =
ph =

Explanation:

To calculate [H⁺] first we calculate the total number of H⁺ ions.

H⁺ from HCl ⇒ 49.3 mL * 1.19 gSolution/mL * 38 gHCl / 100 gSolution = 22.29 g HCl

H⁺ from HNO₃ ⇒ 19.5 mL * 1.42 gSolution/mL * 70 gHCl / 100 gSolution = 19.38 g HNO₃

Total H⁺ moles = 0.612 + 0.308 = 0.920 mol H⁺

Final Volume = 1.00 L

Now we calculate pH:

To calculate [OH⁻], we calculate pOH:

pOH = 13.964 = -log[OH⁻]

bcde is the incorrect answer it is a

i belive it is water