Question: Calculate the pH of a solution with a hydrogen ion concentration of 0.00001 M. pH: 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...
Calculate the pH of a solution that is 0.50 M {eq}CH_3NH_2 {/eq} and 0.70 M {eq}CH_3NH_3Cl {/eq}. pH: The concentration of hydrogen ions or hydronium ions varies inversely with the pH. The higher the concentration of hydrogen ions in a solution, the lower will ...
Calculate the pH of a solution that is 0.5 M {eq}CH_3COOH {/eq} and 0.5 M {eq}CH_3COONa {/eq}. Buffer Solution: A buffer solution is a solution of a weak acid and its conjugate base or a weak base and its conjugate base. In this case, the concern of having a re...
Calculate the pH of a solution sontaining 0.085M nitrous acid( HNO2,Ka=4.5x10^-4) and 0.10M potassium nitrite( KNO2). 扫码下载作业帮拍照答疑一拍即得 答案解析 查看更多优质解析 举报 1,科学家在森林中发现了一个孔雀石(碱式碳酸铜).森林火灾后,孔雀石走了,但在明亮的红色固体的余烬中发现的,它是...
5. Calculate the pH of the solution when samevolume of 0. 25 mol dm-3 HClO4 solution and0. 40 mol dm-3 HNO3 solution are mixed. 答案 0.49相关推荐 15. Calculate the pH of the solution when samevolume of 0. 25 mol dm-3 HClO4 solution and0. 40 mol dm-3 HNO3 solution are mixed....
Calculate the pH of an aqueous solution with {eq}\left [ OH^- \right ] = 4.1 \times 10^{-11} {/eq} M at 25 degrees Celsius. pH: The acidity and basicity of aqueous solution are quantitatively represented by pH. This value is obtained when {eq}\rm{[H_3...
M HCl solution . Video SolutionMore from this Exercise17 videos Text SolutionVerified by Experts Note. At the first instance, it appears that as [H+]=10−8, therefore, pH should be 8. But pH cannot be 8 but should be less than 7 because the solution is acidic. The reason is that...
What are the resulting concentrations of acetic acid (henceforth called AcHAcH), Ca2+CaX2+ and acetate (henceforth called Ac−AcX−, and what is the resulting pHpH? KaKa(acetic acid) = 1.75×10−5.1.75×10−5. My attempted solution: This problem gives me two equilibr...
Calculate the pH for each of the following: a) 0.10 M aniline (C6H5NH2) solution (Kb=4.3x10-10 b)0.10 M C6H5NH3Cl solution (Kb=4.3x10-10 Attempt: Well I'm having a hard time figuring out which both of those substances dissociate too. Part A I think I have worked out properly ...
Apply the formula: pH = ½(pKa - log a) pKa = 4.65 a = 0.050 mol dm–3 pH = ½(4.65 – log (0.05)) pH = ½(4.65 – (–1.30)) pH = ½(5.95) = 2.98 or 3.0 Note that this is a solution of a weak acid so it is not surprising that the pH is < 7. 暂无解析...