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1. Why does an oil-and-vinegar salad dressing have two separate layers? 2. What is meant by...
please help me answer the questions with the provided data. Data Table for Part 4 s-soluble,...
please help me answer the questions with the provided
data.
Data Table for Part 4 s-soluble, ss-slightly soluble, i-insoluble mass of beaker 205.354 mass of beaker + 10.0mL. NaCI 1A 56 Water Oil Type of particle(s) present (molecule, ion, both) Polarity of solute L NaCI 1a 563 g CuSO mass of beaker + dry NaCl mass of solution mass of solute (NaC1) sucrose ar vegetable oils 11.609 g vinegar 3-268 Part 2 S-strong electrolyte, W-weak electrolyte, N- non-clectrolyte 1. Calculate...
What does it mean to "standardize" a solution? Why is this important? 1. Last week you...
What does it mean to "standardize" a solution? Why is this important? 1. Last week you created a triangular phase diagram for use in understanding ternary mixtures. This is a common application in geology. Consider the diagram below and the numbered points. a. What is the composition at point 12? b. If a tie-line were to be drawn that connected points 10-13-12-14, what would you 2. interpret it to mean? Sandstone 9100% 80% 40% 12- 60% 40% 13 20 %...
chem 110 experiment 12 tritation vinegar need help fast please!!! The density of vinegar is 1.01...
chem 110 experiment 12 tritation vinegar
need help fast please!!!
The density of vinegar is 1.01 g/mL. How would this information
affect your experimental results.
2. Weak acids, such as acetic acid, typically have an odor, whereas
strong acids often do not. Explain this is so
EXPERIMENT # 1 2 ACETIC ACID CONTENT OF VINEGAR Objectives Use chemical pll indicators to find endpoints of acid base titrations Use the burets to undertake chemical titrations PreLab questions i. Lab. If commercial...
need help for these questions thank you 1. What is the concentration (in M) of an...
need help for these questions
thank you
1. What is the concentration (in M) of an aqueous solution of sulfuric acid prepared by transferring 25.0 mL of 6.00 M H2So4(aq) to a 250 mL-volume volumetric flask that is subsequently filled to its 250 mL-mark with distilled water? 2. What volume of a saturated solution of 8.43 M KI(aq) at 20 C is needed to form 10.0 L of a 1.00 M solution? What volume of pure water is needed as...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
with steps 6) Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water our homes? 7) List and explain the 3 partcles and 1 ray given off in ra...
with steps
6) Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water our homes? 7) List and explain the 3 partcles and 1 ray given off in radioactive decay and explain what they come from if necessary. Also explain the effect on the nucleus when each decay happens. 8) If the solubility limit of sodium acetate (Molar mass 82 g/mol) at room temp is 76 grams per 100 grams of water,...
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting. 4.2. Def fin...
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting. 4.2. Def fine the terms strong electrolyte and weak electrolyte. Give an example of each 4.3. Ex plain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound. 4.4. What are the advantages and disadvantages of using a molecular equation to represent an i reaction? 4.5. What is a spectator ion? IlIlustrate with a complete ionic reaction 4.6. What...
please help with my pre lab additional information Pre-Lab Questions: 1. What is the definition of...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what volume of the titrant (in mL) must be added to completely neutralize the acid? Show all of your work (including the chemical equation). (1 point) Post-lab Questions: Experiment #9: Acid-Base Titrations Student Learning Objectives : Students will gain practice with the accurate preparation of solutions. Students will perform acid-base titrations and prepare titration curves. Students will identify strong and weak acids by the shapes...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased decreased not affected 2. A supersaturated solution may be prepared by slowly cooling down a solution saturated at an elevated temperature. TRUE FALSE 3. A dilution is a solution made by adding a solvent to a supersaturated solution. TRUE FALSE 4. When sugar & water are mixed, a clear liquid results. In this scenario, the sugar is considered a Solute Solution Solvent All of...
please help me answer the questions with the provided
data.
Data Table for Part 4 s-soluble, ss-slightly soluble, i-insoluble mass of beaker 205.354 mass of beaker + 10.0mL. NaCI 1A 56 Water Oil Type of particle(s) present (molecule, ion, both) Polarity of solute L NaCI 1a 563 g CuSO mass of beaker + dry NaCl mass of solution mass of solute (NaC1) sucrose ar vegetable oils 11.609 g vinegar 3-268 Part 2 S-strong electrolyte, W-weak electrolyte, N- non-clectrolyte 1. Calculate...
What does it mean to "standardize" a solution? Why is this important? 1. Last week you created a triangular phase diagram for use in understanding ternary mixtures. This is a common application in geology. Consider the diagram below and the numbered points. a. What is the composition at point 12? b. If a tie-line were to be drawn that connected points 10-13-12-14, what would you 2. interpret it to mean? Sandstone 9100% 80% 40% 12- 60% 40% 13 20 %...
chem 110 experiment 12 tritation vinegar
need help fast please!!!
The density of vinegar is 1.01 g/mL. How would this information
affect your experimental results.
2. Weak acids, such as acetic acid, typically have an odor, whereas
strong acids often do not. Explain this is so
EXPERIMENT # 1 2 ACETIC ACID CONTENT OF VINEGAR Objectives Use chemical pll indicators to find endpoints of acid base titrations Use the burets to undertake chemical titrations PreLab questions i. Lab. If commercial...
need help for these questions
thank you
1. What is the concentration (in M) of an aqueous solution of sulfuric acid prepared by transferring 25.0 mL of 6.00 M H2So4(aq) to a 250 mL-volume volumetric flask that is subsequently filled to its 250 mL-mark with distilled water? 2. What volume of a saturated solution of 8.43 M KI(aq) at 20 C is needed to form 10.0 L of a 1.00 M solution? What volume of pure water is needed as...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
with steps
6) Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water our homes? 7) List and explain the 3 partcles and 1 ray given off in radioactive decay and explain what they come from if necessary. Also explain the effect on the nucleus when each decay happens. 8) If the solubility limit of sodium acetate (Molar mass 82 g/mol) at room temp is 76 grams per 100 grams of water,...
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting. 4.2. Def fine the terms strong electrolyte and weak electrolyte. Give an example of each 4.3. Ex plain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound. 4.4. What are the advantages and disadvantages of using a molecular equation to represent an i reaction? 4.5. What is a spectator ion? IlIlustrate with a complete ionic reaction 4.6. What...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what volume of the titrant (in mL) must be added to completely neutralize the acid? Show all of your work (including the chemical equation). (1 point) Post-lab Questions: Experiment #9: Acid-Base Titrations Student Learning Objectives : Students will gain practice with the accurate preparation of solutions. Students will perform acid-base titrations and prepare titration curves. Students will identify strong and weak acids by the shapes...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased decreased not affected 2. A supersaturated solution may be prepared by slowly cooling down a solution saturated at an elevated temperature. TRUE FALSE 3. A dilution is a solution made by adding a solvent to a supersaturated solution. TRUE FALSE 4. When sugar & water are mixed, a clear liquid results. In this scenario, the sugar is considered a Solute Solution Solvent All of...
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