![SOLVED: What is the pH of a 0.15 M NH4OH solution with a Kb of 1.78x10^-5? a) 12.09 b) 11.93 c) 10.85 d) 11.21 SOLVED: What is the pH of a 0.15 M NH4OH solution with a Kb of 1.78x10^-5? a) 12.09 b) 11.93 c) 10.85 d) 11.21](https://cdn.numerade.com/previews/296d2161-2d87-4d49-9df4-49f1dd432945.gif)
SOLVED: What is the pH of a 0.15 M NH4OH solution with a Kb of 1.78x10^-5? a) 12.09 b) 11.93 c) 10.85 d) 11.21
Welcome to Chem Zipper.com......: Calculate the emf of the cell: Pt H2(1atm)ICH3COOH(0.1M) II NH4OH(0.01M)IH2(1 atm)Pt and Ka for CH3COOH= 1.8x10^-5 and Kb for NH4OH = 1.8x10^-5
![Ka for CH3COOH is 1.8xx10^(-5) and Kb for NH4OH is 1.8xx10^(-5) The pH of ammonium acetate will be : Ka for CH3COOH is 1.8xx10^(-5) and Kb for NH4OH is 1.8xx10^(-5) The pH of ammonium acetate will be :](https://d10lpgp6xz60nq.cloudfront.net/ss/web/1046555.jpg)
Ka for CH3COOH is 1.8xx10^(-5) and Kb for NH4OH is 1.8xx10^(-5) The pH of ammonium acetate will be :
![Sebanyak 0,1 mol NH4OH (Kb = 10-5) di campurkan dengan 0,05 mol NH4Cl hingga volume 1 liter - Mas Dayat Sebanyak 0,1 mol NH4OH (Kb = 10-5) di campurkan dengan 0,05 mol NH4Cl hingga volume 1 liter - Mas Dayat](https://blogger.googleusercontent.com/img/b/R29vZ2xl/AVvXsEgHnhbWQfrVLUVIZNpZNCRrMPu5ounLNaE-ZTN577wNqPJgl5sglxU8R3pzmTGJXWaRwHAGODzbLKYBv8F5S2vLhd8brSLr3i8DCHWJTIPZ4yinuG348ASQvB3luWBecX1e_9UoL4Tj9WQboUhqtSEhGqtg5-zvLl8stzWTt47tf5CTBMYZG6Ol9pFp/s806/Screen%20Shot%202022-06-11%20at%2014.10.17.png)
Sebanyak 0,1 mol NH4OH (Kb = 10-5) di campurkan dengan 0,05 mol NH4Cl hingga volume 1 liter - Mas Dayat
Calculate the percentage dissociation of 0.01 M NH4 OH solution. The Kb for NH4OH is 1.75 × 10^(-5). - Sarthaks eConnect | Largest Online Education Community
![SOLVED: Answer the following equation:Ammonium Hydroxide, NH4OH is a weak base. Calculate the pH of 0.60 M solution of ammonium hydroxide. Kb= 1.78 x 10^-5 SOLVED: Answer the following equation:Ammonium Hydroxide, NH4OH is a weak base. Calculate the pH of 0.60 M solution of ammonium hydroxide. Kb= 1.78 x 10^-5](https://cdn.numerade.com/ask_previews/6316e7c4-b8d1-491c-99a5-63f735cd81c0_large.jpg)
SOLVED: Answer the following equation:Ammonium Hydroxide, NH4OH is a weak base. Calculate the pH of 0.60 M solution of ammonium hydroxide. Kb= 1.78 x 10^-5
Welcome to Chem Zipper.com......: What will be the pH of the buffer solution containing 0.15 moles of NH4OH and 0.25 moles of NH4Cl Kb for NH4OH is 1.8x10^-5.
![Concentration of NH4Cl and NH4OH in buffer solution is in the ratio 1:10 Kb for NH4OH is 10^-10 - Chemistry - Electrochemistry - 13532511 | Meritnation.com Concentration of NH4Cl and NH4OH in buffer solution is in the ratio 1:10 Kb for NH4OH is 10^-10 - Chemistry - Electrochemistry - 13532511 | Meritnation.com](https://s3mn.mnimgs.com/img/shared/content_ck_images/ck_5ca769aa95b3b.png)