What is the pH of the solution when 1.48 equivalents of 0.57 M NaOH are added to 467 mL of 1.17 M hydrocyanic acid (HCN,

Business, Finance, Economics, Accounting, Operations Management, Computer Science, Electrical Engineering, Mechanical Engineering, Civil Engineering, Chemical Engineering, Algebra, Precalculus, Statistics and Probabilty, Advanced Math, Physics, Chemistry, Biology, Nursing, Psychology, Certifications, Tests, Prep, and more.
Post Reply
answerhappygod
Site Admin
Posts: 899603
Joined: Mon Aug 02, 2021 8:13 am

What is the pH of the solution when 1.48 equivalents of 0.57 M NaOH are added to 467 mL of 1.17 M hydrocyanic acid (HCN,

Post by answerhappygod »

What Is The Ph Of The Solution When 1 48 Equivalents Of 0 57 M Naoh Are Added To 467 Ml Of 1 17 M Hydrocyanic Acid Hcn 1
What Is The Ph Of The Solution When 1 48 Equivalents Of 0 57 M Naoh Are Added To 467 Ml Of 1 17 M Hydrocyanic Acid Hcn 1 (13.96 KiB) Viewed 11 times
What is the pH of the solution when 1.48 equivalents of 0.57 M NaOH are added to 467 mL of 1.17 M hydrocyanic acid (HCN, K₁= 6.2 x 10-10)? Please give your answer to three decimal places. pH = number (rtol=0.02, atol=1e-08)
Join a community of subject matter experts. Register for FREE to view solutions, replies, and use search function. Request answer by replying!
Top
Post Reply

Return to “Archived Questions & Answers”