Milk of magnesia, Mg(OH)2, is prepared from the reaction of aqueous magnesium sulfate and sodium hydroxide solution. If a solution containing 125 g of MgSO4 is added to a solution with 115 g of NaOH, what is the mass of milk of magnesia produced

Explanation:

Hello.

In this case, since the described chemical reaction between aqueous magnesium sulfate and sodium hydroxide is:

Whereas can see a 2:1 mole ratio between sodium hydroxide and magnesium sulfate whose molar masses are 120.366 g/mol and 39.997 g/mol. Next step, is to compute the yielded moles of milk of magnesia yielded by both 125 g of magnesium sulfate (1:1 mole ratio) and 115 g of sodium hydroxide (2:1 mole ratio):

Thus, since magnesium sulfate yields less moles of milk of magnesia than sodium hydroxide, we infer that MgSO4 is the limiting reactant so the yielded mass of milk of magnesia (58.320 g/mol) is:

Best regards!

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

the link still does not work even when adding it to the url bar

explanation: