If I used 22.7mL of base (1.0M NaOH) for the indicator to change color, how do I find out the concentration of the solution that changed color?
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For this problem you need to use M1V1=M2V2. Your M1 is the 1.0M of NaOH and your V1 is the 22.7mL. All you need is the final volume of the titration when the endpoint is reached and that can be your V2. Then all you have to do is solve of M2 which will be in units of mol/L or M.
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It depends which acid cause you need the ratio in the equation. it's probably HCl if its HCl
HCl + NaOH --> NaCl + H2O
number of moles of base = C*V(IN LITERS)=(22.7/1000)*1.0=0.227mol
n(base)=n(acid) ratio in the equation 1:1
so concentration of acid = n/v
0.227/v( which is your volume of the solution that you put to titrate )
HCl + NaOH --> NaCl + H2O
number of moles of base = C*V(IN LITERS)=(22.7/1000)*1.0=0.227mol
n(base)=n(acid) ratio in the equation 1:1
so concentration of acid = n/v
0.227/v( which is your volume of the solution that you put to titrate )