1. What is the density of a 20 gram of 40 ml liquid?
2. Which liquid would be on top one when one liquid has a density of 1.0
g/cm or .88 g/cm'?
3. Why is the solid phase denser than liquids or gases?
4. How can you witness
5. Balance this equation: H+ = H2O
6. What is the ratio of OH-to H+ in water?
7. What safety equipment should you wear for chemicals?
8. What should you do if chemicals get in your eye during lab?
9. List facts about each of the element group families from 1-18
10. List the ways that matter is measured
11. Define condensation
12. State the kinetic theory of particle movement

1. In order to solve for density, we should know that density is the ratio between mass and volume of a liquid. In this case, we're given both measures: given mass of m = 20 g and volume of V = 40 mL, we may simply apply the equation of density described here:

[tex]d=\frac{m}{V}[/tex]

Substituting the variables, we obtain:

[tex]d=\frac{m}{V}=\frac{20 g}{40 mL}=0.5 g/mL[/tex]

2. Given a mixture of several liquids, it's important to understand that liquids with a greater density will tend to form a bottom layer of a solution, while liquids with a lower density will tend to form a top layer of a solution. Here we have a liquid with a density of [tex]d_1 = 1.0 g/cm^3[/tex] and another liquid with a density of [tex]d_2 = 0.88 g/cm^3[/tex]. Notice that [tex]d_1[/tex] > [tex]d_2[/tex].

This implies that the liquid with a density of [tex]0.88 g/cm^3[/tex] would be on top, as its density is lower than the density of the other liquid with a density of [tex]1.0 g/cm^3[/tex].

3. The solid phase is not always, but typically denser than liquids or gases. There are some exceptions to this rule, for example, ice, a solid phase of water, is less dense than liquid water.

However, for the majority of cases this statement is true. Remember that solid phases are the most ordered phases with atoms being packed closely to each other. In liquids, atoms are more dispersed with distances between them being greater than those in solids. Similarly, gases have the greatest distances between gas atoms among all three phases.

Since density is directly proportional to mass, let's say we take the same volume of a solid, a liquid and a gas. For the same volume, since we'll have a greater number of solid atoms than for a liquid or a gas (because solid atoms are more closely packed with lower average distances between the atoms), the mass to volume ratio will be the greatest for solids.

4. This seems to be an incomplete question.

5. In order to balance the following ionic equation, we need to follow the mass and charge balancing rules. Firstly, expand a water molecule showing the individual parts of it:

[tex]H-OH[/tex]

Secondly, notice that we need to add a hydroxide anion to the proton, so that we obtain the same number of protons and hydroxide anions on the left side, as well as the number of hydrogen and oxygen atoms on the right. This way, the net charge on the left hand side (0) and the net charge on the right hand side (0) are equal, so the charge is balanced as well. We obtain:

[tex]H^+ (aq)+OH^-(aq)\rightleftharpoons H_2O (l)[/tex]

6. We should be familiar with the ionization constant of water in the context of this problem. It is defined as the product between the hydronium ions and hydroxide ions and is a constant number at some given temperature. For pure water, the concentration of hydronium ions is balanced by the concentration of hydroxide anions to yield a neutral pH value, meaning the ratio of one with respect to the other would be 1.

For example, at room temperature, the ionization constant of water is defined as:

[tex]K_w=[H^+][OH^-]=10^{-14}[/tex]

Since we have pure water:

[tex][H^+]=[OH^-]=\sqrt{10^{-14}}=10^{-7}[/tex]

Then the ratio is:

[tex]\frac{[H^+]}{[OH^-]}=\frac{10^{-7}}{10^{-7}}=1

7 to 12. The questions are explained in the file attached.