How Do I Balance calcium bicarbonate reacts with hydrochloric acid ?

Answer 1

#Ca(HCO_3)_2(aq)+2HCl(aq) rarr CaCl_2(aq) +2CO_2(g)uarr+2H_2O(l)#

I believe that here, mass and charge are balanced.

The equation for net ions is...

#HCO_3^(-)+H_3O^(+) rarr CO_2(g)uarr + 2H_2O#
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Answer 2

To balance the chemical equation for the reaction between calcium bicarbonate and hydrochloric acid, we start with the unbalanced equation:

[ \text{Ca(HCO}_3\text{)}_2 + \text{HCl} \rightarrow \text{CaCl}_2 + \text{CO}_2 + \text{H}_2\text{O} ]

Balancing this equation, we see that for every molecule of calcium bicarbonate ((\text{Ca(HCO}_3\text{)}_2)), two molecules of hydrochloric acid ((\text{HCl})) are required to produce one molecule of calcium chloride ((\text{CaCl}_2)), two molecules of carbon dioxide ((\text{CO}_2)), and two molecules of water ((\text{H}_2\text{O})). So the balanced equation is:

[ \text{Ca(HCO}_3\text{)}_2 + 2\text{HCl} \rightarrow \text{CaCl}_2 + 2\text{CO}_2 + 2\text{H}_2\text{O} ]

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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.

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.

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.

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.

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