Question Solved1 Answer Question 14 1 pts What is the pH of a solution be if 7.59 mL of 0.10 M HCl is added to the buffer obtained by mixing 173.38 mL of 0.50 M CH3NH2 and 231.71 mL of 1.0 M CH3NH3CI? (K(CH3NH2) = = 5.2 x 10-4) = 12, enter Input your answer to 2 decimal places. For example, if your answer is pH 12.00

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Transcribed Image Text: Question 14 1 pts What is the pH of a solution be if 7.59 mL of 0.10 M HCl is added to the buffer obtained by mixing 173.38 mL of 0.50 M CH3NH2 and 231.71 mL of 1.0 M CH3NH3CI? (K(CH3NH2) = = 5.2 x 10-4) = 12, enter Input your answer to 2 decimal places. For example, if your answer is pH 12.00
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Transcribed Image Text: Question 14 1 pts What is the pH of a solution be if 7.59 mL of 0.10 M HCl is added to the buffer obtained by mixing 173.38 mL of 0.50 M CH3NH2 and 231.71 mL of 1.0 M CH3NH3CI? (K(CH3NH2) = = 5.2 x 10-4) = 12, enter Input your answer to 2 decimal places. For example, if your answer is pH 12.00
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Molandy ab Hc=0.10Mvolume taken =7.59mlm*mol=M_(xV)=0.10 xx7.59=0.759of KdadderlBuffer of CH_(3)Nth andIt is Basic Buffermmal of CH_(8)NH_(2)=MNV=173.38 xx0.50=86.69m. mal of CrsMH_(3)ar^(-)=231.71 xx10=281.71when Acid is added to Basic Buffer concentration of sat ancreare and that of Base decreale80.0.759m. mal of HCl veact with ... See the full answer