Consider a double replacement reaction between Zinc (ll) chloride and sodium hydroxide: ZnCl2+NaOH ==> Complete the chemical equation by: Be sure to complete step ONE before moving on to the other steps. Break each step down. You should have four steps altogether. 1. Rewriting it to include electrically-neutral ionic product formulas for each formula. Hint for step 1: instead of just writing the product formulas rewrite the entire equation. Concerning the "electrically neutral" part, for example, if Na + Cl2 ==> were your reactants, you would not predict NaCl2 as a chemical product because that is not an electrically neutral compound formula. The Na would have a +1 charge and the Cl would have a -1 charge, 2 (-1) charges would give an overall -2 charge which would not produce an overall 0 charge. Step 2: Balance it. Step 3: Add subscripts (aq, I, s, or g) to show how the reactants combine and which product will precipitate to be collected as a solid. Step 4: Provide subscripts for both reactants and both products.
Consider a double replacement reaction between Zinc (ll) chloride and sodium hydroxide:
ZnCl2+NaOH ==>
Complete the chemical equation by:
Be sure to complete step ONE before moving on to the other steps. Break each step down. You should have four steps altogether.
1. Rewriting it to include electrically-neutral ionic product formulas for each formula.
Hint for step 1: instead of just writing the product formulas rewrite the entire equation. Concerning the "electrically neutral" part, for example, if Na + Cl2 ==> were your reactants, you would not predict NaCl2 as a chemical product because that is not an electrically neutral compound formula. The Na would have a +1 charge and the Cl would have a -1 charge, 2 (-1) charges would give an overall -2 charge which would not produce an overall 0 charge.
Step 2: Balance it.
Step 3: Add subscripts (aq, I, s, or g) to show how the reactants combine and which product will precipitate to be collected as a solid.
Step 4: Provide subscripts for both reactants and both products.
In a balanced chemical equation, the number of atoms on both sides of the equation is equal. A balanced chemical equation follows the law of conservation of mass.
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