Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in this solution are written in the second column of the table. Use the checkboxes to classify each compound. compound HI HF NH3 Na I important species present when dissolved in water H₂O, I, H₂O H₂O, F , HF, H₂O NH,OH ,NH,, H,O Na, I, , H₂O type of compound (check all that apply) ionic molecular strong weak strong weak acid acid base base 0 0 0 0 0 0 0 0 0 0 X S 0

Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in this solution are written in the second column of the table. Use the checkboxes to classify each compound. compound HI HF NH3 Na I important species present when dissolved in water H₂O, I, H₂O H₂O, F , HF, H₂O NH,OH ,NH,, H,O Na, I, , H₂O type of compound (check all that apply) ionic molecular strong weak strong weak acid acid base base 0 0 0 0 0 0 0 0 0 0 X S 0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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You are in a CHML 201 Lab and given two unlabeled beakers: Each beaker contains 50 mL of a clear, colorless, odorless liquid. You are correctly told that one beaker contains a salt water solution of unknown concentration; the other beaker contains pure, distilled water. In a few, clearly written sentences describe two (2) separate lab tests [besides measuring the density] that you could easily and safely perform in order to determine which solution is in which beaker. Describe in detail what lab test you could do, and what results you would observe with each test for each of these two solutions.
Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound HCH, CO₂ 0 0 NH₂ name 0 sodium perchlorate hydrobromic acid 0 type of compound (check all that apply) strong weak strong weak acid acid base base ionic molecular O O O O O O X 5
The maximum contaminant level of cyanide (CN) in drinking water as set by the the Environmental Protection Agency (EPA) is 0.00020 g · L. Express this concentration in parts per million (ppm). Assume the density of water is 1.00 g/mL. concentration: Ppm
A sample of potassium bicarbonate (KHCO3) was reacted with HCl to produce KCl. The following data was collected. Mass of beaker 28.43 g Mass of beaker + KHCO3 36.95 g Volume of HCl 12.0 mL Concentration of HCl 9.0 M Mass of beaker +residue (KCl) 33.82 g Calculate the following quantities. Show calculations where requested: Mass of KHCO3 __________________ Mass of residue __________________ Mass of 1 mol of KHCO3 __________________ No. of moles of KHCO3 used ___________________ Show calculations below No. of moles of HCl added ____________________ Show calculations below: Assuming KHCO3 is the limiting reactant, how many grams of KCl can be formed? Show calculations below: Assuming HCl is the limiting reactant, how many grams of KCl can be formed? Show calculations below: Which reactant is limiting? ___________________ Which reactant is excess? ____________________ Actual yield of KCl: ______________________ Theoretical yield of KCl: ______________________ Percent yield of KCl:…
Solid sodium hydroxide is slowly added to 175 mL of a 0.198 M magnesium bromide solution until the concentration of hydroxide ion is 0.0571 M. The percent of magnesium ion remaining in solution is| 1%. Solid ammonium carbonate is slowly added to 50.0 ml of a 0.118 M barium nitrate solution until the concentration of carbonate ion is 0.0440 M. The mass of barium ion remaining in solution is grams.
Matti is given two bottles of copper(II) sulfate solutions in her senior high chemistry lab. She is told that one bottle contains a saturated solution and the other one contains an unsaturated solution. The solutions are the exact same color and have no particles in the bottles. Describe what Matti can do to distinguish between the two solutions.
Imagine a small amount of each compound in the table below is dissolved in water. Pick the sketch that best shows what the solution would look like, at the atomic level. The large number of faint red and white molecules in the background of each sketch represent the water solvent. Also, the colors of the solute atoms may not mean the same element in each sketch. For example, solute oxygen atoms could be colored yellow in the first sketch but blue in the second. Chlorine atoms could be colored blue in the first sketch but yellow in the second. And so on. Note for advanced students: the sizes of the atoms and any bond angles may not be accurate. pick a sketch compound NaNO, OCI₂ Submit (Drag the slider to choose an image) (Drag the slider to choose an image)
A student places 20.00 mL of 0.1005 M HCl in a flask and adds a few drops of phenolphthalein. She adds a NaOH solution of unknown molarity to a buret and records the initial reading as 1.50 mL. She adds the NaOH solution from the buret to the HCI solution until a pale pink color is obtained and records the final buret reading as 22.00 mL. What is the molarity of the NaOH solution? Show your calculations. 2. 53
The stock solution in the stock beaker contains 10.00 mL of 0.1000 M iron(III) nitrate solution, 10.00 mL of 0.1000 M potassium thiocyanate solution, and 10.00 mL of 0.5000 M nitric acid solution. What is the total volume of the stock solution? How many moles of iron (III) nitrate are present in the stock solution? How many moles of potassium thiocyanate are present in the stock solution? Based on the moles of iron (III) nitrate and moles of potassium thiocyanate, how many moles of iron (III) thiocyanate do you expect to be formed Once you determine the moles of iron (III) thiocyanate formed, determine the concentration of iron (III) thiocyanate in the final solution.
Imagine a small amount of each compound in the table below is dissolved in water. Pick the sketch that best shows what the solution would look like, at the atomic level. The large number of faint red and white molecules in the background of each sketch represent the water solvent. Also, the colors of the solute atoms may not mean the same element in each sketch. For example, solute oxygen atoms could be colored yellow in the first sketch but blue in the second. Chlorine atoms could be colored blue in the first sketch but yellow in the second. And so on. Note for advanced students: the sizes of the atoms and any bond angles may not be accurate. compound BaCl, CO pick a sketch (Drag the slider to choose an image) (Drag the slider to choose an image) X $ Education All Rights Reserved of the 1 Privacy
Suppose a student performs a similar reaction using sodium bicarbonate (NaHCO3) instead of sodium carbonate. The sodium bicarbonate is dissolved in water, and a solution of 6.0 M HCl is added to the sodium bicarbonate in increments. Bubbles are observed during the reaction. The data collected is shown in the table. moles of NaHCO3: mass of empty beaker (g) moles of NaCl: mass of beaker and NaHCO3 (g) initial volume of 6.0 M HCl (mL) How many moles of NaHCO3 were used? balanced equation: final volume of 6.0 M (ml) mass of beaker and NaCl (g) How many moles of NaCl were produced by the reaction? Write the balanced chemical equation for the reaction. Include physical states. 84.000 g 86.279 g 20.0 mL 12.0 mL 85.585 g mol mol
Virtual graduate student Sherry Molestonecraft is assigned to help you carry out the standardization of your NaOH solution. She weighs out 1.30 grams of solid KHP (molar mass 204.2 g/mol) and dissolves it in about 50 mL of water in an Erlenmeyer flask. She then titrates the KHP solution to the equivalence point using the NaOH solution described in Question 1 above. The volume of NaOH solution needed to reach the equivalence point is 34.41 milliliters. This is a practice question that i need help with. thank you