What is the [OH–] in the mixture?
how do i do this?
Relationships that you will need:
75ml=75 x 10^-3L
50ml=50 x 10^-3L
Moles=Molarity*Volume(L)
Molarity*Volume(L)=0.200 M NaOH*50 x 10^-3L=0.01 moles of NaOH
Molarity*Volume(L)=0.100 M NaOH*75 x 10^-3L=0.0075 moles of NaOH
Total moles of NaOH=0.01+ 0.0075 = 0.0175 moles of NaOH
Total volume=75 x 10^-3L +50 x 10^-3L=125 x 10^-3 L
[OH–]= M of NaOH= total moles/total volume (L)
[OH–]=0.0175 moles/125 x 10^-3 L=0.14M
[OH–]=0.140 M
*****Answer must contain 3 significant figures
M1V1 + M2V2 = M3V3
(0.200 mol/L) (50.0 mL) + (0.100 mol/L) (75.0 mL) = (x) (125 mL)
x = 0.140 M
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Verified answer
Relationships that you will need:
75ml=75 x 10^-3L
50ml=50 x 10^-3L
Moles=Molarity*Volume(L)
Molarity*Volume(L)=0.200 M NaOH*50 x 10^-3L=0.01 moles of NaOH
Molarity*Volume(L)=0.100 M NaOH*75 x 10^-3L=0.0075 moles of NaOH
Total moles of NaOH=0.01+ 0.0075 = 0.0175 moles of NaOH
Total volume=75 x 10^-3L +50 x 10^-3L=125 x 10^-3 L
[OH–]= M of NaOH= total moles/total volume (L)
[OH–]=0.0175 moles/125 x 10^-3 L=0.14M
[OH–]=0.140 M
*****Answer must contain 3 significant figures
M1V1 + M2V2 = M3V3
(0.200 mol/L) (50.0 mL) + (0.100 mol/L) (75.0 mL) = (x) (125 mL)
x = 0.140 M