Sodium hydroxide and magnesium chloride react as shown by this equation: 2naoh + mgcl2 → mg(oh)2 + 2nacl. suppose the reaction begins with 637 milliliters of 1.35 m sodium hydroxide solution and excess magnesium hydroxide. what is the theoretical yield of magnesium hydroxide if the resulting solution has a volume of 2.82 liters? use the periodic table and the polyatomic ion resource. the mass of magnesium hydroxide formed is grams

- 25.1 g

Solution:- The balanced equation is:

From given balanced equation, there is 2:1 mol ratio between sodium hydroxide and magnesium hydroxide.

From given molarity and volume, we calculate the moles of NaOH and using mol ratio the moles of magnesium hydroxide are calculated that could easily be converted to grams on multiplying by it's molar mass.

Molar mass of magnesium hydroxide  = 24.305 + 2( 15.999 + 1.008)

= 24.305 + 2(17.007)

= 58.319 gram per mol

let's make the set up using dimensional analysis as:

=

So, 25.1 grams of magnesium hydroxide are formed.

passing a magnet thought the

mixture , because iron gets attracted to magnet .

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.