The discussion revolves around the solubility product constant (Ksp) of silver sulfate (Ag2SO4) and its calculations. The solubility of silver sulfate is established at 1.3 x 10^-6 mol/L at 20 degrees Celsius. The Ksp expression is defined as Ksp = [Ag+]^2[SO4^2-], leading to a calculated Ksp value of 1.7 x 10^-12. Participants also explore related concepts such as electrochemical cells, ion separation procedures, and the calculation of hydronium ion concentration in acetic acid solutions.
PREREQUISITESChemistry students, educators, and anyone involved in analytical chemistry or chemical education will benefit from this discussion, particularly those focusing on solubility and electrochemistry.
correct, what about molarity and what would you do with it to find the Hydronium concentration at equilibrium?yoshi6 said:60.05 g/mol i think
yep ... and have you read when you can neglect x = the concentration change?yoshi6 said:oh so that is where you got x^2/ [1.2/60.05]...
1AM, i'im so bored, lol. what time is it there?yoshi6 said:okay, makes sense, I'm just curious, what time is it over there?
naw idc, i want to be a chem tutor @ my school but i don't think i'll get hired b/c they prefer to hire professionals :( so I'm happy to help because i really don't want to forget what i learned, and i have no motivation to review on my own.yoshi6 said:wow...2am, I have been doing homework for hours...thank you so much for your help! I feel like I owe you a present
i go to a CC in Houston, lol ima PM u because i don't think they'd like chattingyoshi6 said:I should but I don't think I am going to yet...what school do you go to?