What is the principle behind this test? Add 5 drops of 10% sodium hydroxide and 1 drop of 0.5%...
Question:
What is the principle behind this test? Add 5 drops of 10% sodium hydroxide and 1 drop of 0.5% copper sulfate to 5 drops of the liver of pig in a sucrose solution.
Carbohydrates
Carbon, oxygen, and hydrogen-containing biomolecules associated with the function of energy storage and an important part of the structural components of the cellular organization are called carbohydrates and the simplest domain of the carbohydrates which cannot be broken/hydrolyzed further is called the monosaccharides.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerIt is given that "add 5 drops of 10% sodium hydroxide and 1 drop of 0.5% copper sulfate to 5 drops of the liver of pig in a sucrose...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:

from
Chapter 4 / Lesson 9Learn about carbohydrates, a type of organic molecule and source of energy. Probe the difference between simple carbohydrates and complex carbohydrates. Discover what foods contain carbohydrates and how the body uses them.
Related to this Question
- Suppose you suspect that your unknown is either copper (II) nitrate or copper (II) sulfate. You decide to add NaOH to your known as a test reagent. Will this test distinguish between the two possibili
- I have test procedure to evaluate the clarity of a sodium hydroxide (NaOH) sample that goes like this: Dissolve 10g of NaOH in carbon dioxide free water and dilute to 100ml with the same solvent. Please explain how to perform this test.
- A few drops of water were added to a test tube containing 0.5 grams of anhydrous copper sulfate (CuSO4) and the following observations were noted. Anhydrous copper sulfate: light blue Anhydrous copper sulfate plus water: sky blue What can you conclude fro
- A student is asked to prepare 250.0 mL of 3.5 M copper (II) sulfate from solid copper (II) sulfate pentahydrate. Describe how this solution should be made in the chemistry laboratory.
- A student used the following steps in testing for a non-sugar solution. I. Add Benedict's solution to the non-sugar solution. II. Added diluted HCl to the non-sugar solution and boiled it. III. Added NaOH solution to the non-sugar solution in (II) and b
- Suppose you have placed 20 drops of sodium bisulfate and 3 drops of thymol blue into a well in your well plate. As you add potassium sulfate to the solution, what happens? A. The mixture color changes from red to orange. B. The color becomes faint due to
- What laboratory experiments can be performed to identify key characteristics (and actually identify) unknown metal salts? Activities: 1) Dissolving the unknowns in distilled water and using indicator solution to determine if acidic or basic solution occur
- In the qualitative test for nitrate anion, the test goes like this: Add dilute sodium hydroxide, then add a little aluminum powder. Warm. When describing the test, is it acceptable to use the word "mixture" as in "warm the mixture"?
- As you observed in lab, pellets of sodium hydroxide are very hygroscopic. Describe what happens chemically when a cover is left off of a bottle of NaOH pellets. (Hint: NaOH reacts with carbon ...
- Suppose you were to use 0.1 M potassium hydroxide as the base instead of 0.1 M sodium hydroxide. How would this affect the results of the experiment? A.It would affect the results since the stoichiom
- As you observed in lab, pellets of sodium hydroxide are very hygroscopic. Describe what happens chemically when a cover is left off of a bottle of NaOH pellets. (Hint: NaOH reacts with carbon dioxide
- What test would you need to perform to prove that it is the combination of glucose and the glucose indicator solution that changes color when heated and not just the glucose or the glucose indicator solution alone?
- An aqueous solution of copper (II) sulfate is a thermodynamic system under study. What type of system is this if the solution is contained in a beaker on a laboratory table?
- A student used 5.06 g copper sulphate pentahydrate and salicyclic acid in the performance of the experiment. The student recovered 3.094 g of salicyclic acid and 2.146 g of copper sulphate pentahydrat
- A sample of 1.0 mol dm-3 copper (II) sulfate solution was electrolyzed for 1 hour using copper electrodes. Which change would have caused the largest increase in the amount of copper deposited? a. increasing the concentration of the copper (II) sulfate to
- Timon has tested an unknown sample with Biuret and Benedict's reagents. The solution mixed with Biuret is blue. The solution boiled with Benedict's reagent is also blue. What does this tell Timon about the sample?
- What experiment can you use to (a) separate salt from water? (b) separate iron filings from small pieces of lead? (c) separate elemental sulfur from sugar?
- What assumption(s) must we make in order to be able to calculate the mass of copper metal in a penny using the concentrations of (Cu(NH3)4)2+ determined using the SpectroVis spectrophotometer?
- Explain what is occurring in each of the following procedures or tests from this experiment. (a) Formation of a red precipitate after addition of dimethylglyoxime to a solution. (b) Formation of a
- Which of the following is not suitable for testing the presence of an acid? A) Adding aqueous potassium carbonate. B) Adding aqueous potassium hydroxide. C) Adding Universal Indicator. D) Adding zinc
- Your lab instructor asks you to prepare a series of five standard solutions to be used to make a Beer's Law plot for copper sulfate which is blue-colored. The first solution should be 1/2 the concentr
- Which of the following is NOT valid reasoning for these results: A student begins with 5.00 g of an unknown mixture and recovers 2.91 g of copper sulfate and 2.58 g of salicylic acid? a. One or more of the fractions was not fully dried. b. The mass of t
- 1. In a lab experiment, finding the limiting reactant with sodium bicarbonate and citric acid, it was found that the limiting reactant was sodium bicarbonate. If I have to devise an experiment to test my conclusion to which reactant is limiting do I add s
- A solution is present in a test tube, but the test tube is not labeled. It could be Ni2+ or Mn2+. What reagent could be added to the solution to find out what it contains? Describe what will happen to the solution when the reagent is added if the solution
- What are the 3 possible sources of error when performing a kinetics experiment using a spectrophotometer to determine the transmittance of crystal violet concentration with sodium hydroxide?
- In a lab experiment, copper wire is placed in a cup full copper sulphate. There is also a battery with two wires extending from it, a red on and a black one. Then, the different wires / leads of the 9 V battery are touched to the copper wire, one at a tim
- In a laboratory experiment, a 10.0Ml sample of sodium chloride solution is poured into an evaporating dish with a mass of 24.10g. The combined mass of the evaporating dish and the sodium chloride is 36.15g. After heating, the evaporating dish and sodium
- An unlabeled bottle containing a solution was found in the lab. It contains one of the following: AgNO3, CaCl2, or Al2(SO4)3. Describe how you would test the solution to determine which solution it is
- What substance is present if the FeCl3 test gives a purple color? Which sample is the most impure?
- What are three possible errors in an experiment using KHP for standardization of NaOH? Indicate how the error would affect final results or conclusion of the experiment.
- An unknown hydrate of copper (II) oxalate is to be identified in the lab. What is it? The following data was collected by a student: Mass of crucible = 23.776 g Mass of crucible + hydrate = 24.889 g M
- Predict what is present in each of the following: a. A solution that turns orange-red when mixed with Benedict's reagent and heated for 5 min.... b. A solution that turns blue-black when mixed with
- When setting up their experiment, a student discovered that the solution in their flask turned bright pink upon adding 2 drops of the indicator, even before beginning the titration. What do you suspec
- A student is doing the experiment Chemical Formulas of Copper Sulfide by heating copper with excess of sulfur at very high temperatures using a Bunsen burner. Copper and sulfur react stoichiometrically and excess of sulfur escapes from the crucible as sul
- Ten drops of water are added to two small test tubes and to each is added one drop of iodine. The solution turns from a lighter yellow to a darker orange. To one of the test tubes some powdered magnesium is added and mixed well and centrifuged.
- A student is given a sample in lab which contains one of the ions listed below. After adding a few drops of solution to part of the unknown sample, the student got a greyish precipitate. After adding
- A student performing this experiment spilled a small amount of 0.500 M NaOH on the Describe the procedures to be followed to clean up this spill.
- A student is given a sample in the lab which contains one of the ions listed below. After adding a few drops of solution to part of the unknown sample, the student got a greyish precipitate. After add
- What will be wisest to use as a drying agent in the distillation process? a. concentrated phosphoric(V)acid b. sodium hydroxide solid c. anhydrous sodium sulfate d. concentrated sulfuric acid
- You have 4 bottles, each containing roughly 5 grams of a finely powdered white substance. Each bottle contains one of the following: glucose (C6H12O6), sodium chloride (NaCl), aluminum oxide (Al2O3), and zinc sulfate (ZnSO4). Describe the tests that you c
- What possible chemicals can test the presence of limonene except for bromine water and potassium permanganate?
- A 2.50 times 10^{-4} M solution of copper sulfate (blue solution) was analyzed and an absorbance of 0.450 was obtained at a wavelength of 645 nm in a 1.00-cm cuvette. Find the molar absorptivity of the copper sulfate solution.
- An unknown solution gives a brick-red flame test. The solution produces a white precipitate with ammonium carbonate, ammonium sulfate, and ammonium phosphate after heating. Silver nitrate is added to
- Which of the following are solutions? a. Salt/water mixture b. Blueberry muffin c. Brass buckle d. Sand and water mixture
- 4. What is the color change lo be observed between the reaction of crystal violet and sodium hydroxide? 5. Why is it necessary to react the sodium hydroxide in a greater concentration than the concent
- Three colorless solutions are placed in test tubes with no labels. Lying beside the test tubes are three labels: 0.10 M K2CO3, 0.10 M H2SO4, and 0.10 M NaOH. You are to place the labels on the test tubes using only the three solutions. Here are your tests
- Magnesium displaces copper from a dilute solution of copper(II) sulfate; the pure copper will settle out of the solution. A copper(II) sulfate solution is mixed by dissolving 25.000 g of copper(II) sulfate, and then it is treated with an excess of magnesi
- What will be the container for the SN1 reaction? a. Round bottom flask. b. Pasteur pipet. c. Separatory funnel. d. Test tube. e. Graduated cylinder. f. Beaker.
- In a dry evaporating dish, 7.50 g solid copper (II) sulfate pentahydrate was dissolved in 30.0 ml of deionized water at 60.0^\circ C. While stirring slowly 1.23 g of iron powder was added to the solution. The solution was allowed to sit for 10 minutes an
- 1. Colour of original K2Cr2O7 solution: orange Colour after the addition of NaOH: Yellow Colour after the addition of HCl: Orange Direction in which equilibrium is shifted by the addition of: NaOH:
- In a lab experiment, copper wire is placed in a cup full copper sulfate. There is also a battery with two wires extending from it, a red one and a black one. Then, the different wires/leads of the 9V battery are touched to the copper wire, one at a time (
- 3.05 g hydrated copper sulfate produces 1.94 g of anhydrous salt. Assuming complete removal of all water of crystallization, determine the formula of hydrated copper sulfate.
- A student failed to carry out all of the Procedure steps when doing this experiment. Would the following procedural variations result in an experimentally determined molarity of NaOH that is too high
- Beside the usual method of titrating with KMNO_4, what is/are the alternative method/s to test for the presence/amount of oxalate in a compound?
- Which of the following is a heterogeneous mixture? A. air B. sugar dissolved in water C. muddy river water D. brass (an alloy of copper and zinc) E. table salt (sodium chloride)
- 1. In a laboratory experiment, a student was given an unknown compound. After performing the carbohydrate analysis, the student reported the unknown as a reducing aldopentose. *Which tests must have
- 2CrO4^2- (aq, yellow) + 2H3O^+ (aq) <---> Cr2O7^2- (aq, orange) + 3H2O( a) Describe the color change the student should observe after adding excess NaOH to the solution to the equilibrium mixture. b)
- When a drop of BTB (bromothymol blue) solution is added to vinegar, what color does the vinegar turn? a. Yellow b. Green c. Blue d. No change
- What flame test color would be produced for the compound salt substitute with its active ingredient KCl?
- A student who is performing this experiment pours a 6.50 mL sample of the saturated borax solution into a 10-mL graduated cylinder after the borax solution had cooled to a certain temperature T. The student rinses the sample into a small flask using disti
- Explain what affect the following procedural errors would have on the calculated molarity of your fruit juice solution: a. A student failed to allow the volumetric pipette to drain completely when transferring the fruit juice solution to the flask. b. A
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o Ions are displaced from the resin binding sites by any ion that has a higher what?
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o Will the solution coming off of the ion exchange column and collected in a beaker or flask be acidic, basic, or neutral?
- A student measures the potential of a cell made up with 1 M CuSO_4 in one solution and 1 M AgNO_3 in the other. There is a copper electrode in the CuSO_4 and a silver electrode in the AgNO_3 in one so
- Which of the following would be an example of a heterogeneous mixture? a. distilled water b. ocean water c. table salt d. copper
- Can test in the lab Cannot test in the lab Pb(NO3)2 and K2SO4 Ba (NO3) 2 and KOH K2CO3 and KOH K2CO3 and Ni (NO3)2 Ni (NO3)2 and Ba(NO3)2 KOH and K2SO4
- You need to perform gravimetric analysis of a water sample in order to determine the amount of Ag^+ present. (a) List three aqueous solutions that would be suitable for mixing with the sample to perform the analysis. (b) Would adding KNO_3(aq) allow you t
- In the laboratory exercise you will prepare a series of solutions of Cu(NH_3)^2+_4 from a standard solution of copper (II) nitrate. In one experiment a standard solution was prepared by adding 8.00 mL
- What is the percent recovery of the sample if a student dissolves 1.00 g of a mixture of salicylic acid and copper sulfate and recovers 0.62 g and 0.32 g, respectively?
- A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the other. There is a Cu electrode in the CuSO4 and an Ag electrode in the AgNO3. A salt bridge c
- In a simple titration experiment, how and why are the results reproducible?
- Identify these unknown organic compounds: 1. Silver Nitrate test: test with Nitric acid: The reaction mixture remains unchanged 2. Basic Hydrolysis Test: There was no change in the mixture after 2 hours of heating 3. Basic Hydrolysis: Test for ammonia:
- For a laboratory experiment, a student reacts baking sod (NaHCO_3) with 6.00 M vinegar (CH_3COOH) to produce a carbon dioxide (CO_2), sodium acetate (NaCH_3COO) and water (H_2O). (NaHCO_3) + (CH_3COO
- During an experiment on the cycles of copper, a student obtains a percent yield / recovery that is more than 100%. Which of the following observations is not a plausible cause of inflated yield for this experiment? (a) After adding Z n the solution was
- Three colorless solutions in test tubes, with no labels, are in a test tube rack on the laboratory bench. Lying beside the test tubes are three labels: -silver nitrate, AgNO_3 -hydrochloric acid, HCL -sodium carbonate, Na_2CO_3 You are to place the lab
- When 20.9 g of copper (II) sulfate pentahydrate (bluestone) is heated, all the water of hydration is removed from the compound, leaving behind pure anhydrous copper (II) sulfate. What would its dehydrated mass (in g) be? The balanced chemical equation is
- If a student was supposed to pour 3 mL of 0.1 M NH_3/H_2O solution into a test tube to mix with phenolphthalein in order to turn red, but accidentally only poured 1 mL instead, what would happen when phenolphthalein indicator is added?
- Copper container can be used to store (A) Al_2(SO_4)_3 solution. (B) ZnSO_4 solution. (C) FeSO_4 solution. (D) All of these.
- Identify these unknown organic compounds: 1. Acetyl chloride Test: There is no visible change 2. Lucas test: No change was observed 3. Ferric Hydroxamate: A light yellow solution resulted 4. Ferrous Hydroxide Text: A clear yellow solution resulted 5.
- A sample of 32.0 g of aluminum hydroxide, Al(OH)_3 is mixed with a solution that contains 40.0 g of HCl. Identify the limiting reagent.
- A mixture contained aluminum sulfate and sodium sulfate. A sample of the mixture weighing 3.458 g was dissolved in water and treated with sodium hydroxide solution to yield a precipitate. The precipitate was incinerated to yield 0.474 g aluminum oxide. a.
- 1 mL of 0.1 mol/L CuSO4 is mixed with a few drops of concentrated NH3. Then about 1 mL of 1 mol/L HCl is added to the solution. When performed in the lab, the solution went from a light blue to a solution that had a blue precipitate at the bottom, a dark
- 1) A student determines the manganese(II) content of a solution by first precipitating it as manganese(II) hydroxide, and then decomposing the hydroxide to manganese(II) oxide by heating. How many gra
- In the chemical laboratory, the Tollen s test for the presence of reducing sugars (say, in a urine sample) involves treating the sample with silver ions in aqueous ammonia. The result is the formation of a silver mirror within the reaction vessel if a red
- What changes in color of iron nails and copper sulphate solution do you observe after keeping the iron nails dipped in copper sulphate for about 30 minutes?