Please help me these are the only two I have left.
17. If the solubility of a gas is 5.6 g/L at 505 kPa pressure, what is the solubility of the gas when the pressure is 1010kPa? *
19. Calculate the [H⁺] for the aqueous solution in which [OH⁻] is 1 x10⁻⁹. Is this solution acidic, basic or neutral? Show your work *
17. If the solubility of a gas is 5.6 g/L at 505 kPa pressure, what is the solubility of the gas when the pressure is 1010kPa? *
The solubility of a gas is directly proportional to the pressure; i.e., the more pressure the higher the solubility. So
5.6 g/L x 1010 kPa/505 kPa = ?
19. Calculate the [H⁺] for the aqueous solution in which [OH⁻] is 1 x10⁻⁹. Is this solution acidic, basic or neutral? Show your work *
(H^+)(OH^-) = Kw = 1E-14
You know OH^- and Kw, solve for H^+.
H^+ > 10^-7 = acid (pH = 0 to 7)
H^+ = 10^-7 = neutral (pH = 7)
H^+ < 10^-7 = basic (pH = 7 to 14)
To solve these two questions, let's break them down step by step.
17. If the solubility of a gas is 5.6 g/L at 505 kPa pressure, what is the solubility of the gas when the pressure is 1010 kPa?
To solve this question, we can use the concept of Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. The equation for Henry's Law is:
Solubility = k * Pressure
Where k is a constant specific to the gas and the solvent.
To find the solubility of the gas when the pressure is 1010 kPa, we can set up a proportion using the given values:
5.6 g/L / 505 kPa = x g/L / 1010 kPa
By cross-multiplying and solving for x, we can find the solubility of the gas when the pressure is 1010 kPa.
19. Calculate the [H⁺] for the aqueous solution in which [OH⁻] is 1 x 10⁻⁹. Is this solution acidic, basic, or neutral?
To find the [H⁺] concentration, we can use the equation for the ion product of water (Kw), which is:
Kw = [H⁺] * [OH⁻]
At 25 degrees Celsius, Kw is equal to 1 x 10⁻¹⁴.
Given that [OH⁻] is 1 x 10⁻⁹, we can rearrange the equation to solve for [H⁺]:
[H⁺] = Kw / [OH⁻]
Plugging in the values, we get:
[H⁺] = (1 x 10⁻¹⁴) / (1 x 10⁻⁹)
Simplifying, we get:
[H⁺] = 1 x 10⁻⁵
This means the concentration of [H⁺] in the aqueous solution is 1 x 10⁻⁵. Since [H⁺] concentration is greater than 1 x 10⁻⁷ (neutral concentration), it can be concluded that the solution is acidic.