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What are some common mistakes students make with stoichiometry of reactions between ions in solutions?

Answer 1

A failure to realize that BOTH mass and charge MUST be conserved in any chemical reaction.

In a chemical reaction, charge must be balanced in addition to mass. For example, if I start with 10 g, I must finish with 10 g. Similarly, if the reactants have a specific charge—positive or negative—the products MUST have the same charge.

As an illustration:

Lead nitrate + sodium chloride #rarr# Lead chloride#darr# + sodium nitrate.

As an equation for net ions:

#Pb^(2+) + 2Cl^(-) rarr PbCl_2(s)darr#

The reactants were neutral (#2^(+) + 2xx1^(-)#); so too the products!

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Answer 2

Serenity Allen

Some common mistakes students make with stoichiometry of reactions between ions in solutions include:

Forgetting to balance the chemical equation properly
Not accounting for the stoichiometry of ions in solution
Incorrectly identifying the reactants and products
Misinterpreting the coefficients in the balanced equation
Failing to convert between units or moles when necessary

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.