(a)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(a)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(b)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(b)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(c)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(c)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(d)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(d)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(e)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(e)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
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Chapter F Solutions
CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- Write the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forwardA student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?arrow_forwardAn aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.arrow_forward
- n general terms, what are the spectator ions in a precipitation reaction? Why are the spectator ions not included in writing the net ionic equation for a precipitation reaction? Does this mean that the spectator ions do not have to be present in the solution?arrow_forwardIn each of the following cases, does a precipitation reaction occur when solutions of the two water-soluble reactants are mixed? Give the formula of any precipitate that forms, and write a balanced chemical equation for the precipitation reactions that occur. (a) sodium carbonate and copper(11) chloride (b) potassium carbonate and sodium nitrate (c) nickel(11) chloride and potassium hydroxidearrow_forwardAqueous solutions of ammonium sulfide and mercury(II) nitrate react and a precipitate forms. (a) Write the overall balanced chemical equation and indicate the state (aq) or (s) for each compound. (b) Name each product. (c) Write the complete ionic equation. (d) Write the net ionic equation.arrow_forward
- A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012 g of barium chromate, BaCrO4. What is the formula of the compound?arrow_forwardOn the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.arrow_forward
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