Aqueous hydrobromic acid is added to a beaker containing solid calcium carbonate. How could the aqueous product here be distinguished from the aqueous product formed if strontium carbonate were substituted for calcium carbonate? i) Balanced equation: ii) Answer:

3. A solution contains silver nitrate, lead (II) nitrate, and calcium nitrate. What reagent could be added to this solution that would separate the calcium nitrate from the other three compounds? Write the formula of the resulting precipitates after the addition of this reagent.

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write the formula and name of the precipitate. (Type your answer using the format CO2 for CO2. Type NONE in the blanks if there is no precipitation reaction.) (a) lead(II) nitrate + potassium bromideformulaname(b) sodium sulfide + nickel(II) sulfateformulaname

8)Does a reaction occur when aqueous solutions of potassium hydroxide and sodium nitrate are combined?   yes or no   If a reaction does occur, write the net ionic equation.

1) Write the type of reaction. 2) Write the chemical equation. Do not worry about balancing this reaction. Just be sure that you have written the correct formulas and states.  solid iron and aqueous copper(II) bromide react to form solid copper and aqueous iron(II) bromide.

Write the balanced equation that occurs when aqueous sodium carbonate reacts with aqueous iron (III) chloride

Magnesium oxide is sometimes used as an antacid to help with indigestion and stomach upset caused by excess stomach acid (hydrochloric acid). Write two balanced chemical equations to  explain how this works. One should be a synthesis and the other a neutralization.

14.4 g of magnesium nitrate is dissolved in 1.20 L of water. 25 mL of this solution is taken and diluted to 175 mL with water. What is the final concentration of the nitrate ion?

All ionic compounds dissolve in water.  True  False

A precipitation reaction involves the formation of a precipitate when aqueous solutions are mixed. Not all combinations of aqueous solutions produce precipitates, and it is important to be able to predict the ones that do. A) Complete and balance the molecular equation for the reaction between aqueous solutions of lithium fluoride and potassium chloride, and use the states of matter to show if a precipitate forms. B) Write the complete ionic equation for the reaction that takes place when aqueous solutions of lithium fluoride and potassium chloride are mixed.   C) Write the net ionic equation for the precipitation reaction, if any, that may occur when aqueous solutions of lithium fluoride and potassium chloride are mixed. If there is no net ionic equation, simply write "none."