181

You visited us 181 times! Enjoying our articles? Unlock Full Access!

Potassium Dichromate

QUES: Calcula...

Question

QUES: Calculate the Ph of a 10^-5M HCl solution if 1ml of it is diluted to 1000ml , K_w= 1× 10^-14.

Open in App

Solution

moles =Molarity volume in liters
=10^-5mol/L0.001L
=1.010^-8moles

please note M stands formolarity and its unit is mol/L

M of final solution =moles/volume in L

=1.010^-8moles/1L
HCl(aq)===>H+(aq) +Cl-(aq)

molarity of HCl and H+ are same since mole ratio is 1:1

pH=-log[H+]
pH=-log(1.0*10^-8)
=-(-8)
=8

you can also find the conc of final solution usign dilution formula
M1V1=M2V2

Suggest Corrections

Similar questions

10^{- 5}

(K_{w} = 10^{- 14} a n d l o g (10.5) = 1.02

H C l

p H = 5

1 m L

1

p H

p H

H C l

6.95

H C l

[\begin{matrix} 10^{- 6.95} = 11.22 \times 10^{- 8} 10^{- 7.05} = 8.90 \times 10^{- 8} \end{matrix}]

p H

N H_{4} C l

K_{b} = 1.0 \times 10^{- 5}

K_{w} = 1.0 \times 10^{- 14}

Join BYJU'S Learning Program