If 50.0 mL of a 0.75 M hydrochloric acid solution is titrated with 1.0 M sodium hydroxide, what is the pH after 10.0 mL of NaOH have been added

Explanation:

moles of hydrochloric acid = 50 x 10⁻³ x .75 = 37.5 x 10⁻³ moles in HCl solutions.

moles of NaOH in its solution = 10 x 10⁻³ x 1 moles = 10 x 10⁻³ moles .

10 x 10⁻³ moles  of NaOH will neutralise 10 x 10⁻³ moles of HCl .

HCl remaining = (37.5 - 10 ) x 10⁻³ moles = 27.5 x 10⁻³ moles

volume of solution = 50 + 10 = 60 mL = 60 x 10⁻³ L

molarity of remaining HCl = 27.5 x 10⁻³ / 60 x 10⁻³

= .4583 M .HCl

concentration of H⁺ = .4583 M

pH = - log ( .4583 )

= .34 .

your mom.com . : 0000

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.