The student titrated 10 ml of standered 0.15 M HCl with his sodium hydroxide solution. When the titration reached the equivalence point, the student found that he had used
10.3 ml of Sodium hydroxide solution. Calculate the molarity of the sodium hydroxide solution.

0.15 M

Explanation:

Step 1: Write the neutralization reaction

NaOH + HCl ⇒ NaCl + H₂O

Step 2: Calculate the moles of HCl that reacted

10 mL of 0.15 M HCl was used. The moles of HCl that reacted are:

Step 3: Calculate the moles of NaOH that reacted

The molar ratio of NaOH to HCl is 1:1. Then, the moles of NaOH that reacted are 1.5 × 10⁻³ moles.

Step 4: Calculate the concentration of NaOH

1.5 × 10⁻³ moles of NaOH are in 10.3 mL of solution. The molarity of NaOH is:

65uuyhjghj8ykitdyidii

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.