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option c. is correct
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What do the conjugates of hydrochloric acid, hydrobromic acid, hydroiodic acid, nitric acid and perchloric acid...
answer all 4 please!!! What volume of a 0.263 M perchloric acid solution is required to...
answer all 4 please!!!
What volume of a 0.263 M perchloric acid solution is required to neutralize 22.5 mL of a 0.150 M calcium hydroxide solution? mL perchloric acid What volume of a 0.122 M potassium hydroxide solution is required to neutralize 16.2 mL of a 0.288 M hydrochloric acid solution? mL potassium hydroxide An aqueous solution of calcium hydroxide is standaridized by titration with a 0.199 M solution of hydroxide acid. If 12.6 mL of base are required to...
1. Write the balanced equation for the reaction between calcium carbonate and hydrochloric acid in water,...
1. Write the balanced equation for the reaction between calcium carbonate and hydrochloric acid in water, generating aqueous calcium chloride and liberating carbon dioxide gas. (You will need this for Part 1 of the experiment!) 2. Calculate the concentration of one liter of the resulting calcium chloride solution (assuming you started with 102.7 mg of calcium carbonate) in units of molar and millimolar. Also calculate the concentration in "parts-per-million as CaCO3". (Refer to section 13.5 of your textbook, if needed.)...
What is a good hypothesis for this lab?? I need to write one. Acid Base lab INSTRUCTIONS Acid-bas...
what is a good hypothesis for this lab?? I need to write one. Acid Base lab INSTRUCTIONS Acid-base indicators are used to let you know whether the solution you are working with is acidic or basic. We have many acid-base indicators available to us today, but the first indicators were made from natural compounds. The indicator that you will be making comes from purple cabbage and is simply called cabbage extract indicator. Procedure: Goggle red cabbage as an acid-base indicator....
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid....
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid. The exceptions are silver ion, Ag mercurous ion, Hg,: and lead(II) ion, Pb. Consequently, the addition of HCI to a solution of metal cations leads to the selective precipitation of these three ions. While the theory behind the separation and identification of these ions has been outlined in the general discus- sion of the qualitative analysis scheme, some aspects of this chemistry need to...
Titration: Acids and Bases 2. How can you determine which acid is diprotic? 3. using the...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
It's a weak acid strong base titration Experiment 4: Identification of an unknown acid by titration...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
Standardization of NaOH: Acid Base Titration Objective: In this lab, you will accurately determine the concentration...
Standardization of NaOH: Acid Base Titration Objective: In this lab, you will accurately determine the concentration of a solution of sodium hydroxide (NaOH) using a 0.500M potassium hydrogen phthalate (KHP) standard solution. Background: Acid–Base Titrations When an acid reacts with a base, a neutralization reaction occurs. The H+ ions from the acid and the HO– ions from the base combine to form water and are therefore neutralized. The other product of reaction is a salt. For example, hydrochloric acid reacts...
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...
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4...
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4 to 1.00 L B) dissolving 46.7 g of K2SO4 in water and diluting to 500.0 ml, then diluting 25.0 ml of this solution to a total volume of 500.0 mL C) dissolving 46.7 g of K2SO4 in water and diluting to a total volume of 250.0 mL D) dilution of 1.00 mL of 0.355 M K2SO4 to 1.00 L E) diluting 46.7 mL of...
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...
answer all 4 please!!!
What volume of a 0.263 M perchloric acid solution is required to neutralize 22.5 mL of a 0.150 M calcium hydroxide solution? mL perchloric acid What volume of a 0.122 M potassium hydroxide solution is required to neutralize 16.2 mL of a 0.288 M hydrochloric acid solution? mL potassium hydroxide An aqueous solution of calcium hydroxide is standaridized by titration with a 0.199 M solution of hydroxide acid. If 12.6 mL of base are required to...
1. Write the balanced equation for the reaction between calcium carbonate and hydrochloric acid in water, generating aqueous calcium chloride and liberating carbon dioxide gas. (You will need this for Part 1 of the experiment!) 2. Calculate the concentration of one liter of the resulting calcium chloride solution (assuming you started with 102.7 mg of calcium carbonate) in units of molar and millimolar. Also calculate the concentration in "parts-per-million as CaCO3". (Refer to section 13.5 of your textbook, if needed.)...
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid. The exceptions are silver ion, Ag mercurous ion, Hg,: and lead(II) ion, Pb. Consequently, the addition of HCI to a solution of metal cations leads to the selective precipitation of these three ions. While the theory behind the separation and identification of these ions has been outlined in the general discus- sion of the qualitative analysis scheme, some aspects of this chemistry need to...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
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...
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4 to 1.00 L B) dissolving 46.7 g of K2SO4 in water and diluting to 500.0 ml, then diluting 25.0 ml of this solution to a total volume of 500.0 mL C) dissolving 46.7 g of K2SO4 in water and diluting to a total volume of 250.0 mL D) dilution of 1.00 mL of 0.355 M K2SO4 to 1.00 L E) diluting 46.7 mL of...
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...
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