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Data Table for Part 4 s-soluble,...
question 9.5) can someone please explain to me why CaCO3 is soluble in water and not...
question 9.5)
can someone please explain to me why CaCO3 is soluble in water
and not carbon tetrachloride (CCl4)? thank you ?!
9.35 9.50 9.379.39 9.67 9.41 9.43 9.459.479.499.55 9.57 9.1 Identify the solute and the solvent in each solution composed of the following: a. 10.0 g of NaCl and 100.0 g of H, O b. 50.0 mL of ethanol, C, H, O, and 10.0 mL of H, O c. 0.20 L of O, and 0.80 L of N2 9.5...
SOLUTIONS 22. Non-polar compounds are soluble in ionic compounds b) electrolytes c) polar solvents d) non-polar...
SOLUTIONS 22. Non-polar compounds are soluble in ionic compounds b) electrolytes c) polar solvents d) non-polar solvents 23. Which of the following would increase the solubility of gaseous O2 in water? (there is more than correct answer, mark them all!) Decreasing the temperature of the solution Increasing the temperature of the solution Decreasing the pressure of the solution Increasing the pressure of the solution 24. Which of the following describes an unsaturated solution? A solution that has less than the...
please help me answer question 1 to 3, thank you Chapter 9, Solutions, Review & Extra Credit. 2 Points for each XC c...
please help me answer question 1 to 3,
thank you
Chapter 9, Solutions, Review & Extra Credit. 2 Points for each XC correct answer; 6 points total, max. Partial Credit given. Suggestions...work in teams [it will improve the learning experience] 1. Solutions-A solution forms when a solute (the smaller quantity) dissolves in a solvent (the larger quantity). In a solution, the particles of solute are evenly distributed in the solvent. A solute may be a gas, liquid or solid. A...
Need help doing chem calc. Please help! Additional Problems Show all work and calculations! 1. Identify...
Need help doing chem calc.
Please help!
Additional Problems Show all work and calculations! 1. Identify the following as a weak electrolyte, strong electrolyte, or nonelectrolyte and write the equation for when they are in solution. Example: PbCl2 is a weak electrolyte PbCl2(s)く-) Pb2+(aq) +2 Cl-(aq) a. H2SO4 c. H3PO4 d. (NH4)3PO4 e. CH3C2OH f. Ba(OH)2 g. CH3CO2H h. HCI 2. Calculate the concentration of a solution in which 5.8 moles of NaCl are dissolved in 250 mL of solution'?...
Please walk me step by step on how to get the calculated pH for the weak...
Please walk me step by step on how to get the calculated pH
for the weak acid. I dont understand this at all and really need
step by step not just a brief explanation. Thank you
A pH of Acid Solutions: 1. Strong Acid Measured pH [HCI), 1.48 0.10M [HCI), 2.17 0.010M Molarity (0.0 (1.0) -M2 (10.00 Calculated pH 1.00 2.00 10o = 0.01 -log(0.01)=2 [HC,H,O, Kas 1.8x10s Weak Acid Measured pH [HC,H,O, 3.44 0.01M Molarity 0.10M Calculated pH Compare...
Please help me with questions 7-12.Thanks Part 1: Observations, Data and Calculations 1. In the table,...
Please help me with questions 7-12.Thanks
Part 1: Observations, Data and Calculations 1. In the table, describe your observations when the different solutes were dissolved in tap water and when vinegar was added into the solution. (2 marks) Table 1: Solubility and reactivity Solute Solubility in water Reactivity with vinegar Baking soda Sugar Salt 2. (1.5 marks) Write a chemical equation to represent what you observed when you added each solute to water. 3. (0.5 mark) Write a chemical equation...
Hope the genius can help me those questions. Thanks ♥️ Name 1. Definitions. Fill in the...
Hope the genius can help me those questions.
Thanks ♥️
Name 1. Definitions. Fill in the blank with the LETTER of the most appropriate term from the following A. Bronsted-Lowery acid C. strong acid E. weak electrolyte G. weak acid I. Arrhenius acid B. D. electrolyte base H. ions J. Arrhenius base L. autoionization of water N. Boyle's Law P. Charles Law S. pressure V. manometer X. Dalton's Law K. hydronium ion M. pH scale O. combined gas law R....
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of...
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of 0.12 M LIOH solution. What is the molarity of the unknown HSO, solution (in MJ? (Write the balanced reaction first) A. 0.20 M B. 0.40 M C. 0.10 M D. 0.36 M E. 0.25 M 22. Complete and balance the following acid-base reaction. What volume of 0.200 M HCI is required for the complete reaction of 1.00 g of Ca(OH): (FW - 74.10g/mol? Ca(OH)(s)...
LAB VII. PRACTICE PROBLEMS - CHAPTER 4 NAME: SECTION: b) How many grams of strontium nitrate,...
LAB VII. PRACTICE PROBLEMS - CHAPTER 4 NAME: SECTION: b) How many grams of strontium nitrate, Sr(NO), are needed to prepare 3.40x10 ml. of a 0.925 M solution? c) To what volume should 50.0mL of a 6.00M HCI stock solution be diluted to obtain a 1.50M HCl solution? How much water should be used? d) A 38.5ml sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate...
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the so...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
question 9.5)
can someone please explain to me why CaCO3 is soluble in water
and not carbon tetrachloride (CCl4)? thank you ?!
9.35 9.50 9.379.39 9.67 9.41 9.43 9.459.479.499.55 9.57 9.1 Identify the solute and the solvent in each solution composed of the following: a. 10.0 g of NaCl and 100.0 g of H, O b. 50.0 mL of ethanol, C, H, O, and 10.0 mL of H, O c. 0.20 L of O, and 0.80 L of N2 9.5...
SOLUTIONS 22. Non-polar compounds are soluble in ionic compounds b) electrolytes c) polar solvents d) non-polar solvents 23. Which of the following would increase the solubility of gaseous O2 in water? (there is more than correct answer, mark them all!) Decreasing the temperature of the solution Increasing the temperature of the solution Decreasing the pressure of the solution Increasing the pressure of the solution 24. Which of the following describes an unsaturated solution? A solution that has less than the...
please help me answer question 1 to 3,
thank you
Chapter 9, Solutions, Review & Extra Credit. 2 Points for each XC correct answer; 6 points total, max. Partial Credit given. Suggestions...work in teams [it will improve the learning experience] 1. Solutions-A solution forms when a solute (the smaller quantity) dissolves in a solvent (the larger quantity). In a solution, the particles of solute are evenly distributed in the solvent. A solute may be a gas, liquid or solid. A...
Need help doing chem calc.
Please help!
Additional Problems Show all work and calculations! 1. Identify the following as a weak electrolyte, strong electrolyte, or nonelectrolyte and write the equation for when they are in solution. Example: PbCl2 is a weak electrolyte PbCl2(s)く-) Pb2+(aq) +2 Cl-(aq) a. H2SO4 c. H3PO4 d. (NH4)3PO4 e. CH3C2OH f. Ba(OH)2 g. CH3CO2H h. HCI 2. Calculate the concentration of a solution in which 5.8 moles of NaCl are dissolved in 250 mL of solution'?...
Please walk me step by step on how to get the calculated pH
for the weak acid. I dont understand this at all and really need
step by step not just a brief explanation. Thank you
A pH of Acid Solutions: 1. Strong Acid Measured pH [HCI), 1.48 0.10M [HCI), 2.17 0.010M Molarity (0.0 (1.0) -M2 (10.00 Calculated pH 1.00 2.00 10o = 0.01 -log(0.01)=2 [HC,H,O, Kas 1.8x10s Weak Acid Measured pH [HC,H,O, 3.44 0.01M Molarity 0.10M Calculated pH Compare...
Please help me with questions 7-12.Thanks
Part 1: Observations, Data and Calculations 1. In the table, describe your observations when the different solutes were dissolved in tap water and when vinegar was added into the solution. (2 marks) Table 1: Solubility and reactivity Solute Solubility in water Reactivity with vinegar Baking soda Sugar Salt 2. (1.5 marks) Write a chemical equation to represent what you observed when you added each solute to water. 3. (0.5 mark) Write a chemical equation...
Hope the genius can help me those questions.
Thanks ♥️
Name 1. Definitions. Fill in the blank with the LETTER of the most appropriate term from the following A. Bronsted-Lowery acid C. strong acid E. weak electrolyte G. weak acid I. Arrhenius acid B. D. electrolyte base H. ions J. Arrhenius base L. autoionization of water N. Boyle's Law P. Charles Law S. pressure V. manometer X. Dalton's Law K. hydronium ion M. pH scale O. combined gas law R....
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of 0.12 M LIOH solution. What is the molarity of the unknown HSO, solution (in MJ? (Write the balanced reaction first) A. 0.20 M B. 0.40 M C. 0.10 M D. 0.36 M E. 0.25 M 22. Complete and balance the following acid-base reaction. What volume of 0.200 M HCI is required for the complete reaction of 1.00 g of Ca(OH): (FW - 74.10g/mol? Ca(OH)(s)...
LAB VII. PRACTICE PROBLEMS - CHAPTER 4 NAME: SECTION: b) How many grams of strontium nitrate, Sr(NO), are needed to prepare 3.40x10 ml. of a 0.925 M solution? c) To what volume should 50.0mL of a 6.00M HCI stock solution be diluted to obtain a 1.50M HCl solution? How much water should be used? d) A 38.5ml sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
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