Amanda

How to determine pH for these solutions:

1) [H3O+]=4.2×10−3M

2) [H3O+]=2×10−4M

3) [OH−]=8.9×10−9M

Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation:

CaCO3(s)+2HCl(aq)⟶CO2(g)+H2O(l)+CaCl2(aq)

Tums, an antacid, contains CaCO3. If Tums is added to 10.0 mL of a solution that is 0.350 M in HCl, how many grams of CO2 gas are produced?

In a laboratory experiment, a 19.0 −mL sample of KCl solution is poured into an evaporating dish with a mass of 24.90 g . The combined mass of the evaporating dish and KCl solution is 41.00 g. After heating, the evaporating dish and dry KCl have a combined mass of 28.27 g.

What is the molarity of the KCl solution?

1) 175 g of glucose, C6H12O6, a nonelectrolyte, added to 1.00 kg of water

2) 1.8 moles of CaCl2, a strong electrolyte, dissolved in 1.00 kg of water

3) 65.0 g of LiNO3, a strong electrolyte, dissolved in 1.00 kg of water

Mass of sodium carbonate, 2.3109g

Mass of calcium chloride, 2.2648g

Actual amount of product, 1.63g

Write the balanced chemical equation for the reaction between sodium carbonate and calcium chloride.

1Na2CO3(aq) +1CaCl2(aq) → 2NaCl(s) + 1CaCO3(aq)   (I believe this is right but I am not sure)

1. Calculate the moles of sodium carbonate used

2. Calculate the number of moles of calcium chloride used.

3. Calculate the amount of calcium carbonate that can be made based on the above reactants.

4. Which reactant is limiting, if any?

5. Calculate the percent yield.

During laparoscopic surgery, carbon dioxide gas is used to expand the abdomen to help create a larger working space.

If 4.45 L of CO2 gas at 19 ∘C at 775 mmHg is used, what is the final volume, in liters, of the gas at 41 ∘C and a pressure of 751 mmHg, if the amount of CO2 does not change?

A container is filled with 0.686 g of O2 at 5∘C and 849 mmHg. What is the volume, in milliliters, of the container?

A fire extinguisher has a pressure of 9.0 atm at 25 ∘C. What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 65 ∘C , if volume and amount of gas do not change?

A gas mixture with a total pressure of 5.0 atm is used in a hospital. If the mixture contains 5.9 moles of nitrogen and 1.3 moles of oxygen, what is the partial pressure, in atmospheres, of each gas in the sample?

A hyperbaric chamber has a volume of 1150 L. How many kilograms of O2 gas are needed to give an oxygen pressure of 2.04 atm at 31 ∘C?

In another laparoscopic surgery, helium is used to inflate the abdomen to separate the internal organs and the abdominal wall.

If the He injected into the abdomen produces a pressure of 13 mmHg and a volume of 2.6 L at 30. ∘C, how many grams of He were used?

Consider that 3.30 L of N2, at 25 ∘C and 1.27 atm, is mixed with 2.25 L of O2, at 25 ∘C and 0.468 atm, and the mixture is allowed to react.

N2(g)+O2(g)→2NO(g)

How much NO, in grams, is produced?

If 4.45 L of CO2 gas at 19 ∘C at 775 mmHg is used, what is the final volume, in liters, of the gas at 41 ∘C and a pressure of 751 mmHg, if the amount of CO2 does not change?