The atomic weight of magnesium is 24.305 g/mol. A student weighs out 2,000 g of

Question

The atomic weight of magnesium is 24.305 g/mol. A student weighs out 2,000 g of magnesium. How many moles of Mg are present? When you are performing a titration experiment, how do you know that the reaction is complete and you should slop adding the titrant (what is the signal to stop)? In the elemental stale, copper is a shiny orange-red solid, but in aqueous solution, Cu^+2_(eq) (e.g., CuSO_4_(aq)) is what color? (fill in the blank) An experiment lo determine the unknown concentration of a solution (such as an acid or a base) which uses a buret to measure the volume of the solution the unknown is reacted with is called a In the Production of Hydrogen, the hydrogen gas was generated over (in) water. When the reaction is finished, the TOTAL gas pressure inside the buret is (write in letter) Calculate the formula weight (f_w) of the compound potassium sulfate, K_2SO_4, given the following information: atomic weights K = 39.0983 g/mol, S = 32.066 g/mol, O = 15.9994 g/mol A dye which is dissolved in water, and which changes its color when placed in other solutions of various pH values is a useful solution called an acid-base (one example is phenolphthalein, the substance you used in the titration of vinegar)

Explanation / Answer

(1) Number of moles = weight / gram molecular weight

n = 2.000 / 24.305 = 0.08229mol

(2) During the titration process, an indicator is used which exhibits two different colours in acidic and in base=ic medium. Hence when an equivalent point is reache this indicator changes its colour.

(3) Aqueous CUSO4 solution is in blue colour.

(4) Titrant

(5) (A)

(6) Formula Weight = 2(K) + 1(S) + 4 (O) = 2 ( 39.0983 ) + 1 ( 32.066) + 4 ( 15.9994)

fw = 78.1966 + 32.066 + 63.9976

fw = 174.26 g / mol

(7) An INDICATOR

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