What is the molar concentration of a solution obtained by dissolving 560cm3 of hydrogen chloride gas measured at s.t.p in 92.5cm3 of water.
To solve this problem, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, we need to calculate the number of moles of hydrogen chloride gas (HCl) in 560 cm3 at STP. At STP, 1 mole of any gas occupies 22.4 L of volume. Therefore, the number of moles of HCl is:
n = V / Vm = 560 cm3 / 22.4 L/mol = 0.025 mol
Next, we need to calculate the volume of the solution in liters. We know that 92.5 cm3 of water was used to dissolve the HCl gas. Therefore, the total volume of the solution is:
V = 560 cm3 + 92.5 cm3 = 652.5 cm3 = 0.6525 L
Now we can use the formula to calculate the molarity of the solution:
M = n / V = 0.025 mol / 0.6525 L = 0.038 M
Therefore, the molar concentration of the solution is 0.038 M.
Well, if we're talking about molar concentration, we'll need to dust off our chemistry hats! Are you ready for some hilarious scientific equations?
First things first, we need to establish that the volume of a gas is directly proportional to the number of moles of that gas. Since we have the volume of hydrogen chloride gas, we can calculate the number of moles using the Ideal Gas Law.
Now, the good old Ideal Gas Law is PV = nRT. Since we're dealing with standard temperature and pressure (s.t.p), we can use R as 0.0821 atm·L/mol·K.
But wait, before we go diving into equations, let's convert those volumes to liters. One liter is equal to 1000 cm³, so 560 cm³ is 0.56 L, and 92.5 cm³ is 0.0925 L.
Now we can substitute those values into the equation:
(P * 0.56 L) = (n * 0.0821 atm·L/mol·K * 273.15 K)
To find the molar concentration, we need to know the number of moles of hydrogen chloride gas. So let's solve for "n":
n = (P * 0.56 L) / (0.0821 atm·L/mol·K * 273.15 K)
Now, let's put on our clown noses and calculate the concentration:
n(moles) / Volume(L) = Concentration(molar)
Plug in the values we know, and ka-pow! You'll have your answer, all while chuckling at my chemistry-themed jokes.
To calculate the molar concentration of a solution, we need to know the amount of solute (in moles) and the volume of the solution (in liters).
First, let's find the amount of hydrogen chloride gas (HCl) in moles:
1. Convert the volume of HCl gas from cm³ to liters:
560 cm³ = 560/1000 = 0.56 liters
2. Use the ideal gas law to convert the volume of gas to moles:
At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters.
So, the moles of HCl gas can be calculated as:
Moles of HCl gas = Volume of HCl gas (in liters) / 22.4
= 0.56 / 22.4
≈ 0.025 moles
Next, we need to find the volume of the solution. It is the sum of the initial volume of water and the volume of gas dissolved:
Volume of solution = Volume of water + Volume of HCl gas
= 92.5 cm³ + 560 cm³
= 652.5 cm³
= 652.5/1000 liters
= 0.6525 liters
Now, we can calculate the molar concentration (molarity) using the formula:
Molarity (M) = Moles of solute / Volume of solution (in liters)
Molarity of the solution = 0.025 moles / 0.6525 liters
≈ 0.038 M (rounded to three decimal places)
Therefore, the molar concentration of the solution is approximately 0.038 M.
To find the molar concentration of a solution, you need to know the number of moles of solute and the volume of the solution. In this case, the solute is hydrogen chloride gas, and the solvent is water.
Let's start by finding the number of moles of hydrogen chloride gas. We can use the ideal gas law, which states that the volume of a gas at standard temperature and pressure (STP) is directly proportional to the number of moles of the gas.
According to STP, 1 mole of any gas occupies 22.4 liters. Since we are given the volume of hydrogen chloride gas in cm3, let's convert it to liters.
Given:
Volume of hydrogen chloride gas (V1) = 560 cm3
Volume of water (V2) = 92.5 cm3
1 cm3 = 0.001 liter
V1 (in liters) = 560 cm3 * 0.001 liter/cm3 = 0.56 liter
Now, let's find the number of moles of hydrogen chloride gas using the ideal gas law:
PV = nRT
Where:
P represents the pressure, which is constant at STP (1 atm) and represented as 760 mmHg
V represents the volume in liters (0.56 liters in this case)
n represents the number of moles (what we want to find)
R is the ideal gas constant, which is 0.0821 L·atm/(K·mol)
T is the temperature in Kelvin, which is 273.15 K at STP
Solving for n:
n = PV / RT
n = (1 atm * 0.56 L) / (0.0821 L·atm/(K·mol) * 273.15 K)
n ≈ 0.02506 mol (rounded to five decimal places)
Now we have the number of moles of hydrogen chloride gas. To find the molar concentration, we divide this by the volume of the solution.
Given:
V2 (volume of water) = 92.5 cm3 = 0.0925 L
Molar concentration (C) = n / V2
C ≈ 0.02506 mol / 0.0925 L
C ≈ 0.271 mol/L
Therefore, the molar concentration of the solution obtained by dissolving 560 cm3 of hydrogen chloride gas, measured at STP, in 92.5 cm3 of water is approximately 0.271 mol/L.