The ph of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, ph=−log[h3o+] in neutral solutions at 25 ∘c, [h3o+]=10−7 m and ph=7. as [h3o+] increases, ph decreases, so acidic solutions have a ph of less than 7. basic solutions have a ph greater than 7. the hydroxide and hydronium ion concentrations are related by the the ion-product constant of water, kw , as follows: kw=1.0×10−14=[h3o+][oh−] in the same way as the ph, we can define the poh as poh=−log[oh−]. it follows from the kw expression that ph+poh=14.

1.

2. Acidic: pH < 7.00, neutral: pH = 7.00, basic: pH > 7.00

3. pH + pOH = 14.00 at room temperature

Explanation:

Firstly, it is true that pH is defined as the negative logarithm of the concentration of hydronium ions. A simple rule for any p-function in chemistry is to remember that p = -log. For example:

etc.

Secondly, neutral solutions are the ones which have equal concentrations of hydronium and hydroxide ions regardless of the temperature. At room temperature, specifically, for pure solutions:

Notice that applying the equation above:

This means neutral solutions at room temperature have a pH value of 7.00.

Now, let's say the concentration of hydronium increases to a value of:

Then:

Notice that an increase in the molarity of hydronium lead to a decrease in pH. Therefore, acidic solutions have a pH < 7.00, while basic solutions have a pH > 7.00. Neutral solution was described as the one having pH = 7.00.

Thirdly, ion-product constant of water is defined as:

The given value of:

Is only valid at room conditions. Now let's take the -log of both sides:

Apply the rule of logs:

We obtain:

That said, the equation is proved.

i can ! i just need to know what the paragraph is! : p

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.