18. A solute is the dissolved substance in a solution. A solvent is the major component in the solution. The solvent is often water
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20. Aqueous = a solute dissolved in water NaCl(s) Na + (aq) + Cl - (aq) shows that the ions are dissolved in water This equation for the dissolving of table salt reads… solid sodium chloride yields aqueous sodium ions and aqueous chloride ions.
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22. S olute and solvent particles are in constant random motion, which causes diffusion of the solute into the solvent, resulting in a homogeneous solution.
23. When a solid is in contact with a liquid, at least some small degree of dissolution occurs. Dissolution= dissolving into solution molecules or ions in a solid leave their place in the solid to become surrounded by the solvent
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25. Dissociate = to come apart Dissociation describes the breaking up of an ionic solid.
In a water molecule, the bond polarities are equal, but the two dipoles do not cancel each other because a water molecule is bent. The molecule as a whole is polar. Applying Concepts Which element in water has the higher electronegativity?
The polarity of the water molecule results in hydrogen bonding. a) Partial negative charges are on each oxygen atom; partial positive charges are on the hydrogen atom. b) Because of polarity, hydrogen bonds form. Inferring To form a hydrogen bond, what must be true about the hydrogen and the element to which it is hydrogen bonded?
The polarity of the water molecule results in hydrogen bonding. a) Partial negative charges are on each oxygen atom; partial positive charges are on the hydrogen atom. b) Because of polarity, hydrogen bonds form. Inferring To form a hydrogen bond, what must be true about the hydrogen and the element to which it is hydrogen bonded?
Extensive hydrogen bonding in ice holds the water molecules farther apart in a more ordered arrangement than in liquid water. The hexagonal symmetry of a snowflake reflects the structure of the ice crystal.
A solution cannot be separated by filtration. The small size of the solute particles allows them to pass through filter paper.
When an ionic solid dissolves, the ions become solvated or surrounded by solvent molecules. Inferring Why do the water molecules orient themselves differently around the anions and the cations?
Oil and water do not mix. Oil is less dense than water, so it floats on top. The colors result from the bending of light rays by the thin film of oil.
A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.
A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.
A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.
Water can be driven from a hydrate by heating. a) Heating of a sample of blue CuSO 4 ·5H 2 O begins. b) After a time, much of the blue hydrate has been converted to white anhydrous CuSO 4 .
Water can be driven from a hydrate by heating. a) Heating of a sample of blue CuSO 4 ·5H 2 O begins. b) After a time, much of the blue hydrate has been converted to white anhydrous CuSO 4 .
Deliquescent substances can remove water from the air. a) Sodium hydroxide pellets absorb moisture from the air. b) Eventually a solution is formed. Applying Concepts Identify the solvent and the solute.
Deliquescent substances can remove water from the air. a) Sodium hydroxide pellets absorb moisture from the air. b) Eventually a solution is formed. Applying Concepts Identify the solvent and the solute.
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