Answer to Question #110000 in General Chemistry for eron

Question

(all work above must be complete before attempting the bonus)
You are stuck with a problem. You need to measure pH of a solution known to be made from a metal hydroxide,
but you don’t have a meter or any indicators. You do happen to have some lead (II) nitrate that is soluble, and
you remember that lead (II) hydroxide is insoluble. You add some to 1 liter of your unknown solution and a
precipitate forms. You add more until the precipitate stops forming and then a bit more just in case. After you
filter and dry the precipitate, you have 3.81 grams of it. What was the approximate pH of the original solution?
SHOW YOUR STEPS AND YOUR WORK. EXPLAIN EACH STEP SO I KNOW WHAT YOU DID

Answer 1

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