If 50 mL of 0.1 M HBr is mixed with 50 mL 0.2 M NaOH then find pH of resulting mixture

Question

If 50 mL of 0.1 M HBr is mixed with 50 mL 0.2 M NaOH then find pH of resulting mixture (A) 2.7 (B) 12.7 (C) 10.7 (D) 1.3

Tardigrade Admin · Accepted Answer

underset textbaseN 1 V 1 - underset textacidN 2 V 2= NV NaOH HBr 50 × 0.2 -50 × 0.1= N × 100 =N=(5/100) . [ OH -] =N [ OH -] =5 × 10-2 P OH =- log [ OH -] =- log (5 × 10-2) =2- log 5=2-0.7 P OH = 1.3 P H + P O H =14 P H =14-1.3 P H =12.7

Q. If 50mL of 0.1MHBr is mixed with 50mL0.2MNaOH then find pH of resulting mixture

2.7

12.7

10.7

1.3

baseN1​V1​​−acidN2​V2​​=NV NaOHHBr 50×0.2−50×0.1=N×100 =N=1005​. [OH−]=N [OH−]=5×10−2 POH=−log[OH−] =−log(5×10−2) =2−log5=2−0.7 POH=1.3 PH+POH=14 PH=14−1.3 PH=12.7

Q. If $50 m L$ of $0.1 M H B r$ is mixed with $50 m L 0.2 M N a O H$ then find $p H$ of resulting mixture