Complete the flow chart with the steps necessary for preparing the buffer solutions. in beakers, obtain of the 0.1 m weak acid and of the conjugate base stock solutions. this will be your supply to make the buffer solutions. prepare of the assigned 1: 1 buffer solution in a clean, labeled 100 ml . you will need to use of the 0.1 m weak acid and of the 0.1 m conjugate base. measure out the stock solutions using a clean , being sure to rinse it into the waste beaker between each solution to prevent contamination. in your pre‑lab, write out how much weak acid and conjugate base will be used to make each of the remaining buffer solutions: 1: 4, 1: 9, 4: 1, 9: 1.

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

If 1.8 l of water is added to 2.5l of a 7.0 molarity koh solution, what is the molarity of the new solution

Word equation for k(s)+h2o(l) yield koh(aq) + h2(g)