Balance chemical equation

a. How many milliliters of 1.00 M HCl are needed lớn dissolve 1.00 g of iron (III) hydroxide?b. If you added enough HCl to dissolve the 1.00 g of iron (III) hydroxide and then diluted the solution to 50.0 mL, what would the concentration (molarity) of iron be in the solution?c. How many grams of iron (III) hydroxide can be dissolved in 10.0 mL of 12.0 M HCl?


Acid-Base Titration:

A titration experiment between an acid & a base is the utilization of the neutralization reaction between the protons in the acid solution and the hydroxides in the base solution khổng lồ determine the unknown concentration of the acid or the base.

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In this reaction:

eqFe(OH)_3(s)+ 3HCl (aq) ightarrow FeCl_3 (aq) + 3H_2O(l)/eq

We see that 1 mole of eqFe(OH)_3/eq is reacting with 3 moles of eqHCl/eq to lớn produce 1 mole of eqFeCl_3/eq in the solution.

Question (a.)

The molar amount of 1.00 g of eqFe(OH)_3/eq is:

eq1 / 106.867 = 0.00936 mol/eq

The molar amount of eqHCl/eq needed is:

eq0.00936 * 3 = 0.0281 mol/eq

The volume of eqHCl/eq solution is:

eq0.0281 / 1 * 1000 = oxed28.1 mL/eq

Question (b.)

The molar amount of eqFe(OH)_3/eq is:

eq1 / 106.867 = 0.00936 mol/eq

Thus, the concentration of eqFe^3+/eq in the solution is:

eq0.00936 / 50 * 1000 = oxed0.187 M/eq

Question (c.)

The molar amount of eqHCl/eq is:

eq12.0 * 10 / 1000 = 0.12 mol/eq

The molar amount of eqFe(OH)_3/eq reacting with this amount of eqHCl/eq is:

eq0.12 / 3 = 0.04 mol/eq

Thus, the mass of eqFe(OH)_3/eq is:

eq0.04 * 106.867 = oxed4.27 g/eq


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