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Mercury has a density of 13.6g/mL. What is the mass of 4.72L of mercury?
At what temp would a gas at Standard temp and pressure exert a pressure of 1.20 atm?
1) You are given a mixture of silver and barium carbonate. Which of the following sequences would enable you to obtain a pure sample of silver.
A Add aqueous sodium chloride, filter and crystalize
B Add aqueous sodium chloride, stir and filter
C Add dilute hydrochloric acid, stir and filter
D Add dilute sulfuric acid, stir and filter.
2) Powdered calcium carbonate is commonly placed in chimneys of coal-buring power stations to remove waste gases. Which waste gas will not be removed by the powdered calcium carbonate
A Sulfur dioxide
B Nitrogen Dioxide
C Carbon monoxide
D Phosphorous(V) oxide
My ans for the 2nd Q is C but I am not sure
A Add aqueous sodium chloride, filter and crystalize
B Add aqueous sodium chloride, stir and filter
C Add dilute hydrochloric acid, stir and filter
D Add dilute sulfuric acid, stir and filter.
2) Powdered calcium carbonate is commonly placed in chimneys of coal-buring power stations to remove waste gases. Which waste gas will not be removed by the powdered calcium carbonate
A Sulfur dioxide
B Nitrogen Dioxide
C Carbon monoxide
D Phosphorous(V) oxide
My ans for the 2nd Q is C but I am not sure
What is the molecular weight of the acrylic polymer
A NaOH solution was standardized by titration with a sample of potassium hydrogen phthalate KHC8H4O4 (molar mass= 204.2 g/mol) A sample of pure potassium hydrogen phthalate weighing 3.918 grams was dissolved in water and titrated with the NaOH solution. To reach the equivalence point, 58.90 mL of base was required. (Note: the NaOH and the KHC8H4O4 react in a one to one ratio)
a) How many moles of the solid acid were used in this reaction
b) knowing the acid is monoprotic ( so it will react in a one to one ration with NaOH) how many moles of the base were used in this reaction
c) what was the concentration of the basic solution
a) How many moles of the solid acid were used in this reaction
b) knowing the acid is monoprotic ( so it will react in a one to one ration with NaOH) how many moles of the base were used in this reaction
c) what was the concentration of the basic solution
What does the equation t=pr/nv stand for?
What is the molarity of a solution if 200. mL of solution contains 5.00 g of Na2CO3?
2. A solution is prepared by dissolving 1.50 g of Pb(NO3)2 in a small amount of water and diluting to a total volume of 250.00 mL.
a. Write a chemical equation (with phase symbols) to show what happens to a formula unit of Pb(NO3)2 when it is dissolved in water.
b. What is the molarity of this solution?
c. If a 25.00 mL sample of this solution were removed and diluted to a total volume of 100.00 mL, what would be the molarity of the diluted solution?
a. Write a chemical equation (with phase symbols) to show what happens to a formula unit of Pb(NO3)2 when it is dissolved in water.
b. What is the molarity of this solution?
c. If a 25.00 mL sample of this solution were removed and diluted to a total volume of 100.00 mL, what would be the molarity of the diluted solution?
4. A sample of chlorine gas occupies a volume of 18.35 L at STP. a. How many moles of chlorine are present in this sample?
b. What mass of chlorine gas does this represent?
c. Chlorine gas reacts violently with hydrogen gas to form hydrogen chloride gas. Write a balanced chemical equation for this reaction
d. The sample of chlorine is allowed to react with an excess of hydrogen as described in part (c). How many molecules of hydrogen chloride are formed in this reaction?
e. A solution of hydrochloric acid can be prepared by bubbling hydrogen chloride gas through pure water. If the products of the reaction in part (d) are bubbled through 500.00 mL of water, what is the molar concentration of the hydrochloric acid solution?
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b. What mass of chlorine gas does this represent?
c. Chlorine gas reacts violently with hydrogen gas to form hydrogen chloride gas. Write a balanced chemical equation for this reaction
d. The sample of chlorine is allowed to react with an excess of hydrogen as described in part (c). How many molecules of hydrogen chloride are formed in this reaction?
e. A solution of hydrochloric acid can be prepared by bubbling hydrogen chloride gas through pure water. If the products of the reaction in part (d) are bubbled through 500.00 mL of water, what is the molar concentration of the hydrochloric acid solution?
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How do you find the hydrogen ion concentration with the pH of 5.75?
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#339914 on Dec 2023
#339914 on Dec 2023