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Unit 3 assignment
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Overall expectation 1:1) For each of the following mixtures, explain whether it is a solution (homogeneous mixture)
or a heterogeneous mixture. For the solutions only, identify the solute and the solvent. Cloudy
pond water: Heterogeneous mixture, there are dirt particles floating on top of water that did not
dissolve, solvent is water, solute is dirt particles. Apple juice: Homogeneous mixture, any
particles in apple juice are not visible to the naked eye, solvent is water, solute is all dissolved
substances. Rainwater: Homogeneous mixture, all particles in rainwater are not visible to the
naked eye, solvent is water. 14-karat gold in jewelry: Homogeneous mixture, 14K gold is made
by combining other metals with regular gold to make gold harder, since all the other metals are
not visible to the naked eye; 14 k gold is a homogeneous mixture, solute is the other metals
combined with gold, solvent is gold.
2) Write reactions to show the dissociation into ions of the following substances when they
+ 3−
dissolve in water: Sodium phosphate: 3𝑁𝑎 + 𝑃𝑂4 , Ammonium hydroxide:
+ −
𝑁𝐻4 + 𝑂𝐻
3) Explain why water is such a good solvent for so many different solutes. Water is an excellent
solvent because of its ability to separate electric chargers known as polarity, its ability to form
hydrogen bonds, water makes an excellent solvent and is widely used to dissolve many different
kinds of molecules and substances.
4) Use a solubility table to predict which of the following combinations of compounds would
produce a precipitate. State what the precipitate will be if there will be one. Strontium
hydroxide + ammonium phosphate —> Ammonia + water + strontium phosphate. Strontium
phosphate & ammonia are the precipitates, water will mix in with water. Silver nitrate +
lithium acetate —> Silver acetate + lithium nitrate. All of the elements will dissolve in the
water except for silver which is the precipitate.
5) Write a complete and net ionic equation for the following double displacement
reaction:
Step 1 - Write a balanced equation:
CuNO₃ + KCL → CuCl + KNO₃
Step 2 - Total ionic equation:
+ − + − + − + −
C𝑢 (aq) + NO3 (aq)+𝐾 (aq) +𝐶𝑙 (aq) → 𝐶𝑢 (𝑠) + 𝐶𝑙 (𝑠) + 𝐾 (𝑎𝑞) + 𝑁𝑂3 (𝑎𝑞)
Since all products are soluble and both sides are identical, everything cancels and no reaction
occurs. “No reaction”
6) A conductivity test of a dilute solution of nitrous acid (HNO2 (aq)) has very low electrical
conductivity (the bulb on the tester glows dimly) and the pH is measured to be about 4. The same
concentration of a nitric acid (HNO3 (aq)) solution makes the conductivity tester’s bulb glow
brightly and has a pH of less than 1. Explain the difference between these two acids. The
difference between both of these acids has to do with their ph level. As mentioned in one of the
lessons, substances become more acidic when the ph value gets smaller. Due to this reason, an
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