Consider the following reaction. MgCl2(aq)+2NaOH(aq)⟶Mg(OH)2(s)+2NaC l(aq)

A 156.0 mL solution of 0.234 M MgCl2 reacts with a 42.21 mL solution of 0.849 M NaOH to produce Mg(OH)2 and NaCl.

(a) Caclulate the mass of Mg(OH)2 that can be produced.
(b) The actual mass of Mg(OH)2 isolated was 0.688 g. Calculate the percent yield of Mg(OH)2.

Calculate the ratio of h+ ions to oh– ions at a ph = 7. find the concentration of h+ ions to oh– ions listed in table b of your student guide. then divide the h+ concentration by the oh– concentration. record this calculated ratio in table a of your student guide. compare your approximated and calculated ratios of h+ ions to oh– ions at a ph = 7. are they the same? why or why not? record your comparison in table a. what is the concentration of h+ ions at a ph = 7? mol/l what is the concentration of oh– ions at a ph = 7? mol/l what is the ratio of h+ ions to oh– ions at a ph = 7? : 1

Which metal exist in liquid state and can be cut with knife ?

Sugar is dissolved in water. which is the solute? sugar neither both water