Atmospheric pressure from barometer = (9810) × (13.6) × (0.720) = 96060 Pa = 96.06 kPa Absolute pressure in compartment A, 496.06 kPa P = P + P abs, A gauge, A atm = 400 + 96.06 = Absolute Pressure from barometer
Answer:
i know it is alot but that is how are teacher told us to do, hope this is correct
Explanation:
a. 2.6
b. 12.0
Explanation:
a.
First, we will calculate the molar concentration of HCl.
M = mass of HCl / molar mass of HCl × liters of solution
M = 0.40 g / 36.46 g/mol × 4.5 L
M = 2.4 × 10⁻³ M
HCl is a strong monoprotic acid, so [H⁺] = 2.4 × 10⁻³ M. The pH is:
pH = -log [H⁺]
pH = -log 2.4 × 10⁻³ = 2.6
b.
First, we will calculate the molar concentration of NaOH.
M = mass of NaOH / molar mass of NaOH × liters of solution
M = 0.80 g / 40.00 g/mol × 2.0 L
M = 0.010 M
NaOH is a strong base with 1 OH⁻, so [OH⁻] = 0.010 M. The pOH is:
pOH = -log [OH⁻]
pOH = -log 0.010 = 2.0
The pH is:
14.00 = pH + pOH
pH = 14.00 - pOH = 14.00 - 2.0 = 12.0
Answer:
The amount of sugar in the sample
Explanation:
The independent variable is not dependent on the other observed variable in an experiment. So In this case, it is the amount of sugar as it does not change by the other variable in the experiment, i.e. the number of bees that visit the sample.
The other options are irrelevant in this experiment because they are not being studied.
Chemical properties are those properties that become evident when the material experiences some sort of change. Although there are numerous chemical properties, some most basic ones are <span>reactivity with other chemicals, toxicity, flammability, heat of combustion, oxidation states, chemical stability<span>, types of chemical bonds that will form and others. Unlike physical characteristics that don't change the chemical when altered, changing chemical properties will affect the chemical.</span></span>
When the value of Ksp = 3.83 x 10^-11 (should be given - missing in your Q)
So, according to the balanced equation of the reaction:
and by using ICE table:
Ag2CrO4(s) → 2Ag+ (Aq) + CrO4^2-(aq)
initial 0 0
change +2X +X
Equ 2X X
∴ Ksp = [Ag+]^2[CrO42-]
so by substitution:
∴ 3.83 x 10^-11 = (2X)^2* X
3.83 x 10^-11 = 4 X^3
∴X = 2.1 x 10^-4
∴[CrO42-] = X = 2.1 x 10^-4 M
[Ag+] = 2X = 2 * (2.1 x 10^-4)
= 4.2 x 10^-4 M
when we comparing with the actual concentration of [Ag+] and [CrO42-]
when moles Ag+ = molarity * volume
= 0.004 m * 0.005L
= 2 x 10^-5 moles
[Ag+] = moles / total volume
= 2 x 10^-5 / 0.01L
= 0.002 M
moles CrO42- = molarity * volume
= 0.0024 m * 0.005 L
= 1.2 x 10^-5 mol
∴[CrO42-] = moles / total volume
= (1.2 x 10^-5)mol / 0.01 L
= 0.0012 M
by comparing this values with the max concentration that is saturation in the solution
and when the 2 values of ions concentration are >>> than the max values o the concentrations that are will be saturated.
∴ the excess will precipitate out
