1. Give reasons why the helium atom is smaller than the cesium atom. 2. A student got a problem wrong. They were asked, “How many grams of MgCl2 (molar mass = 95.21 g/mol) are needed to make 3.16 L of a 0.500 M MgCl2 solution?” The correct answer is 150. but the student got 1.58. What mistake did the student make? 3. To solve the following problem what is the reason you must subtract the vapor pressure of water, 24 torr, from the total pressure, 747 torr in order to solve the problem? “A 500.0-mL sample of H2 gas is collected over water at 298 K and 747 torr. What volume would the dry H2 gas occupy at STP? (Given: the vapor pressure of water at 298K is 24 torr).” By the way, the answer is .436 liters. NOTE: I am not asking you to solve this problem. I am asking the reason for subtracting the vapor pressure. If you simply solve the problem, you will get no points.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
1. Give reasons why the helium atom is smaller than the cesium atom.
2. A student got a problem wrong. They were asked, “How many grams of MgCl2 (molar mass = 95.21 g/mol) are needed to make 3.16 L of a 0.500 M MgCl2 solution?” The correct answer is 150. but the student got 1.58. What mistake did the student make?
3. To solve the following problem what is the reason you must subtract the vapor pressure of water, 24 torr, from the total pressure, 747 torr in order to solve the problem?
“A 500.0-mL sample of H2 gas is collected over water at 298 K and 747 torr. What volume would the dry H2 gas occupy at STP? (Given: the vapor pressure of water at 298K is 24 torr).”
By the way, the answer is .436 liters.
NOTE: I am not asking you to solve this problem. I am asking the reason for subtracting the vapor pressure. If you simply solve the problem, you will get no points.
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