题目 Calculate the hydroxide ion concentration, the percent reaction, and the pH of a 0.050 mol×L-1 solution of sodium acetate. (For acetic acid, Ka=1.74×10-5) . 相关知识点: 试题来源: 解析解:NaAc的Kb=101、.00/1.74´105、 = 5.75´101、...
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 7.96 at 25 degrees Celsius. Calculate the hydroxide ion concentration in an aqueous solution with a pH of 8.91 at 25 degrees Celsius. Calculate the hydroxide ion concentration in an aqueous sol...
Since the acid dissociates completely the hydrogen ion concentration is the same as the molarity of the solution. In this case that means the concentration of hydrogen ions, or [H+], is 1.5M. A strong base, on the other hand, has more hydroxide ions than hydrogen ions. Let's say that...
In order to calculate the pH, take the negative log of the hydronium ion concentration. To find the pOH, simply subtract the pH from 14. In order to calculate the pOH, take the negative log of the hydroxide ion concentration. To find the pH, simply subtract pOH from 14. What Do pH a...
Calculate the pH of the given solution whose hydroxide ion concentration is [OH-]=7.4x10-6M Calculate the pH of a solution with a hydroxide ion concentration of 3.8 x 10^8 M. Calculate the pH of a solution with a hydrogen ion concentration of 0.00001 M. Calculate the p...
The pH, which means the power of Hydrogen, is the quantitative expression of the acidity and basicity of a chemical substance.it can be calculated by the concentration of hydrogen ions in the solution through the formula {eq}\rm{pH=-log[H^+]}{/eq}. The usual pH scale...
Through the autoionization of water, we are able to relate the hydronium ion concentration to the hydroxide ion concentration. By extension, this reaction is also used to relate the pH and the pOH of a solution. As such, the calculation of the pH or pOH of a s...
To calculate the pH of a weak acid, it is important to note that pH has no units, thus it is required to define it with H+ ion concentration.
moles = volume x concentration 0.286 x 25 / 1000 = 7.15 x 10^-3 = 0.00715 for potassium hydroxide 0.05 x 50 / 1000 = 2.5 x 10 ^-3 = 0.0025 for sulphuric acid 0.0025 x 2 = 5 x 10 ^-3 = 0.005 so, 0.005 /0.00715 x 100 = 69.9 = 70% ...
The pH will be the total H+H+ concentration, so [H+]=5.624×10−10+0.15[H+]=5.624×10−10+0.15. This is a pH of about 0.823 which is totally wrong. What am I doing wrong? Also, the volumes of the buffer solution or of the acid solution have not been given....