When 100 mL of 0.4 M `CH_3COOH` are mixed with 100 mL of 0.2 NaOH, the `[H_3O^+]` in the solution is approximately : `[K_a(CH_3COOH)=1.8xx10^(-5)]`

When 100 ml of 0.4 M CH_3 COOH is mixed with 100 ml of 0.2 M NaOH , the [H_3O]^(+) in the solution is approximately : [K_a (CH_3COOH)= 1.8 xx 10 ^(-5) ]

When 100ml of 0.4M \(CH_{3}COOH\) is mixed with 100ml of 0.2M NaOH,the [H3O]+" in the solution is approximately "[Ka(CH3COOH)=\(1.8\times10^{-5}\)

100 ml of 0.1 M CH_(3)COOH are mixed with 100ml of 0.1 M NaOH , the pH of the resulting solution would be

100 ml of 0.2 M CH_3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be ( pKa of CH_3COOH=4.76 )

100 ml of 0.2 M CH3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be (pKa of CH3COOH=4.76)

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

0.1M CH_(3)COOH(aq.) Is mixed with 0.1M NaOH(aq.). The pH of solution on mixing will be ( K_(a) of CH_(3)COOH is 1.8xx10^(-5)

If 50 ml 0.2 (M) CH_3COOH is mixed with 20 ml 0.2 (M) NaOH solution, then what will be the pH of the mixed solution?