When Crush Davis placed a drop of a metal ion solution onto a metal square, how will he know that...
Question:
When Crush Davis placed a drop of a metal ion solution onto a metal square, how will he know that a reaction has occurred?
A. A white precipitate
B. An astringent smell
C. Color change of the solution metal ions
D. A dark spot on the metal under the solution
E. Bubbles indicating the formation of a gas
Chemical reaction
The occurrence of a chemical reaction is verified by observing the physical as well as chemical changes. The former is generally observed by the difference in the shape and size of the reactant wheres the latter is observed by the formation of precipitate or gas formation.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerIt is given that "Davis placed a drop of a metal ion solution onto a metal square", The change in the color of the solution confirms the...
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:
Get access to this video and our entire Q&A library
Chemical Reactions in Everyday Life
from
Chapter 13 / Lesson 3
51K
Learn about chemical reactions in everyday life. Understand there are many chemical reactions in everyday life and discover some examples of chemical changes.
Related to this Question
- For the reaction converting the CuSO_4 solution to metallic copper with Zinc, how do you know when enough Zinc has been added? a.The reaction will start to bubble aggressively. b. The reaction will turn from blue to colorless. c. The solution will turn
- A piece of copper is immersed in a solution of oxygenated water. What would you expect to observe as this reaction proceeds? a. a precipitate forms b. a gas is produced c. a blue color appears in the solution d. the blue color in the solution disappears
- A solid sample of metal is dropped into an acidic solution. Bubbles form as the metal is dissolved. What kind of reaction have you likely observed?
- how will you recognize that a single replacement has occurred when you combine a) an active metal with 6M HCL b)an active metal with CuSO4 solution
- When a copper wire is placed into a silver nitrate solution, silver crystals and copper (II) nitrate solution form. If 57.1 g silver is actually recovered from the reaction, determine the percent yiel
- [Cu(H2O)6]2+ and [Cu(NH3)4]2+ both appear blue in solution because of the presence of copper ions. However, the two solutions are not identical. How would the appearance of these solutions differ? If given an unlabeled sample of each, how could
- During the preparation of a brass solution, suppose a trace of some other metal ion that absorbs at 620 mu enters the solution. Would this cause the percent copper found to be higher, lower, or equal to the percentage of copper in the brass sample?
- When metal X is placed in a solution of Y2+, the surface of metal X changes color. When metal Y is placed in acid solution, colorless gas bubbles form on the surface of the metal. When metal X is placed in a solution of Z2+, no change is observed in the s
- What happens when you heat aqueous copper nitrate? What color does the solution turn?
- A sensitive test for bismuth(III) ion consists of shaking a solution suspected of containing the ion with a basic solution of sodium stannite. A positive test consists of the formation of a black precipitate of bismuth metal. Stannite ion is oxidized by b
- A sample of water was observed to have peculiar taste. The taste may be caused by chloride ions or sulphate ions. How can you determine which ion is responsible for the taste? Identify which solutions you would need for your experiment and the precipitate
- Consider the following reaction: FeSCN^{2+} (aq) (red) to Fe^{3+} (aq) (pale yellow ) + SCN^- (aq) (colourless) The solution was initially dark red in color. If some Ag^+ were added to the solution to form AgSCN(s), what would happen to the color of the s
- How could a student use the color change property of iron (III) chloride to monitor when the reaction had reached competition? a. She could have placed a drop of iron (III) chloride directly in the reaction mixture and waited until the color disappeared.
- When a metal is placed in water, what is experimental evidence that a reaction occurred? A. pink color of solution upon addition of phenolphthalein B. bubbles C. a solid precipitate forms D. both A and B E. none of the above; metals do not react with wate
- In the last reaction of the copper cycle, students observe a blue solution turning colorless. What does this signify about the reaction that is occurring?
- When two solutions are mixed and a new color is observed, is this color change an indication that a chemical reaction has occurred? Explain.
- A Precipitate is: a. A solid formed from a chemical reaction b. A rocky edge c. A substance dissolved in a liquid e. A change in solution colour during a chemical change
- 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
- Aluminum sulfate, known as cake alum, has a remarkably wide range of uses, from dyeing leather and cloth to purifying sewage. In aqueous solution, it reacts with base to form a white precipitate. (a)
- Which of the following process are spontaneous? (a) Salt dissolves in H_2O (b) A clear solution becomes a uniform color after a few drops of dye are added. (c) Iron rusts.
- If a piece of copper metal is dipped into a solution containing Cr^{3+} ions, what will happen?
- You added sodium sulfate solution to well A1 and observed a color change. Select the answer that best explains how your observations tell you which way the equilibrium is shifting. (Well A1 has 10 dro
- A chemist wants to extract copper metal from copper chloride solution. The chemist places 1.5 grams of aluminum foil in a solution of 14 grams of copper (II) chloride. A single replacement reaction takes place. What best explains the state of the reaction
- If you submerge a silver teaspoon in copper sulfate solution, what reaction would you expect and why?
- A student begins with 9.7 mL of a 0.20 M CuSO_4 solution and performs the reaction shown. She recovers 0.073 grams of copper metal. CuSO_4 (aq) + Zn (s) to Cu (s) + ZnSO_4 (aq) a. What is the theoretical yield of copper in grams? b. What is the actual yie
- How can one know the possible ways to distinguish solutions made up of different ions?
- 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
- A student begins with 10.4 mL of a 0.27 M CuSO_4 solution and performs the reaction shown. She recovers 0.074 grams of copper metal. CuSO_4 (aq) + Zn (s) to Cu (s) + ZnSO_4 (aq) a. What is the theoretical yield of copper in grams? b. What is the actual yi
- What would you observe and see at the end of the reaction of zinc and lead nitrate? Include information about color changes and bubbles. zinc + lead nitrate arrow zinc nitrate + lead
- If an aluminum strip were placed in a tin(II) solution, what would you observe? A. The aluminum strip would dissolve B. Tin metal will plate out on the aluminum strip C. No reaction D. A and b
- When a piece of copper wire is placed in a colorless solution of silver nitrate, the surface of the wire becomes coated with a shiny silvery material, and the copper begins to form aqueous copper(II) nitrate, which is blue. Which of the following statemen
- A dilute aqueous solution of PtCl4 is a pale yellow to colorless, but a concentrated solution is a deep red. What explanation can you give for this behavior?
- In an experiment, ferric ions were reacted with thiocyanate. How might the results differ if ferrous ions were used instead?
- Keeping in mind that aqueous the copper(II) ion is blue and the aqueous zinc ion is colorless, predict what you would observe over a several-day period if: A strip of Cu is placed into a beaker containing aqueous zinc ions.
- A solution is known to contain either Bi^{3+} ion or Cd^{2+} ion. Describe a single test that would determine which ion is present. Explain what you would expect in each case.
- A student tried to recover all the gold metal from a 1.738 M solution of gold (III) sulfate by adding magnesium metal. They started with 450 gal of solution and added 65 lb of magnesium metal. When the reaction was complete, they recovered 150 lb gold met
- Keeping in mind that aqueous the copper(II) ion is blue and the aqueous zinc ion is colorless, predict what you would observe over a several-day period if: A strip of Zn is placed into a beaker containing aqueous zinc ions.
- What is the color of light absorbed by an aqueous solution of CuSO4?
- A cloudy, colloidal precipitate of Agl forms in a solution containing Nal and excess AgNO_3. How would you describe the surface of the growing colloidal precipitate? a. A positive surface from adsorb
- In an experiment using fertilizer, the gravimetric method is used. The reaction solution is tested with litmus paper to determine when a solution has become basic enough that it will be able to precipitate. NH3 is added until the red litmus paper turns bl
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o What color is a solution containing Cu2+ ions?
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o What color is a solution containing H+ ions?
- Explain what would happen to the color of a dilute solution containing FeCl_4^-, if you added a solution of sodium chloride, NaCl.
- A solution is known to contain Bi^3+ ion or Cd^2+ion or both. Describe the test(s) that could be used to separate and identify these ions. Describe the results you would expect to see for each ion, if
- A sulfide ion can be confirmed by adding few drops of NaOH and a sodium nitroprusside solution to a sodium carbonate extract, which results in a violet color. The violet color is due to a) Na2[Fe(CN)5NO] b) Na4[Fe(CN)5NOS] c) Na3[Fe(CN)6]
- A student is given a sample in lab which contains one of the ions listed below. After adding a few drops of AgNO_3 solution to part of the unknown sample, the student observed a greyish precipitate. After adding a few drops of Mg(NO_3)_2 solution to anoth
- There are two possible methods for recovering copper from a solution of copper (II) sulfate; one uses precipitation and the other uses redox. Copper (II) ions can be precipitated as copper (II) carbonate. CuSO4(aq) + Na2CO3(aq) arrow CuCO3(s) + Na2SO4(aq)
- A solution containing an ionic compound is subjected to anion and cation confirmation tests, providing the following results. Addition of silver nitrate: a bright yellow precipitate formed Flame test: a purple color was observed Identify the ionic compoun
- Shaun's Chemistry class did flame testing with the following metal ions: Sodium (Na^+1), Barium (Ba^2+), Calcium (Ca^2+), Copper (Cu^2+), Potassium (K^+1), Strontium (Sr^2+), Lithium (Li^+1) Explain the effect of the nitrate ion solution on the color emi
- A student tried to recover all the gold metal from a 1.738 M solution of gold (III) sulfate by adding magnesium metal. They started with 450 gal of solution and added 65 lbs of magnesium metal. When the reaction was complete, they recovered 150 lbs of gol
- 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
- Red scale residue (COPPER II) partly dissolves in dilute acid to form a pale blue solution. Name the pale blue solution
- A student dissolved a piece of copper wire, then converted it to CuO, filtered the CuO from solution, and determined the mass of the CuO. The CuO was then dissolved, reduced to copper metal, and recov
- A solution containing an ionic compound is subjected to the anion and cation confirmation tests, providing the following results: Addition of silver nitrate: a bright yellow precipitate formed Flame test: a purple color was observed Identify the ionic com
- Determine the difference between a solid that has crystallized from solution versus one that has precipitated from solution. Assume the solid has already come out of solution and that you did not observe the process but were given an Erlenmeyer flask with
- Small pieces of silver, copper, and magnesium are placed in solutions that contain one of the following ions: Ag^+, Cu^{2+}, and Mg^{2+}. The metal/solution combinations tested are summarized in the following table. Any reaction that occurred followed the
- A beaker is found to contain I^-(aq), Cu^{2+}(aq), and\ Mg^{2+}(aq) ions with Ag(s). A strip of aluminum metal is added to the beaker. What would you observe?
- If you put copper metal into a solution of aluminum sulfate, what would happen?
- There are two possible methods for recovering copper from a solution of copper(II) sulfate, one uses precipitation and the other uses redox. (a) Copper(II) ions can be precipitated as copper(II) carbo
- A commercial for a well known cleaning powder says that it "shakes out white, then turns blue" what type of reaction is occurring? What compound can one use to produce this effect?
- 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
- 2.00 liters of 0.580 M CuSO4 solution is electrolyzed by passing 1.70 amps through the solution for 2.00 hr using inert electrodes. What is the Cu2+ in the solution at the end of the electrolysis
- Which of these changes are chemical changes? a silver teapot turns black. sugar crystals are ground to a fine powder. two clear colorless salt solutions are mixed and a bright orange precipitate fo
- a) If sodium hydroxide (NaOH) is added to the solution, will a color change be observed? b) If so, how does the addition of sodium hydroxide result in a color change? Explain by showing the effect of the addition of NaOH on the equilibrium for the reacti
- What would happen if a solution of NaOH was added to CuSO_4?
- A solution is known to contain Bi3+ ion or Cd2+ ion or both. Describe the test(s) that could be used to separate and identify these ions. Describe the results you would expect to see for each ion if t
- A student tried to recover all the gold metal from a 1.738 M solution of gold (III) sulfate by adding magnesium metal. They started with 450 gal of solution and added 65 lbs of magnesium metal. When the reaction was complete, they recovered 150 lbs gold m
- 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
- A greenish-blue salt known to be composed of copper and chloride ions is dissolved in DI water. Aluminum metal is used to reduce the copper ions to metallic, copper, which is then collected, dried, and weighed. If the original sample has a mass of 1.362 g
- Suggest a way to determine if colorless liquid in a beaker is water. How could an experimenter discover if there is salt dissolved in the water?
- What will be observed if red and blue litmus papers were dipped into the solution after electrolysis?
- A student did not rinse the volumetric flask out after preparing the standard nickel ion solution. The student used the same volumetric flask to prepare the solution of the unknown nickel ion. How wil
- Were the solids that formed when the MgSO4 solution was added to the detergent solution the result of a physical or chemical change?
- A strip of zinc metal was placed in a beaker that contained 120mL of a solution of copper(2) nitrate, Cu(NO_3)_2(aq). The mass of the copper produced was 0.813g. Find the initial concentration of the
- A test tube has a solution of KMnO4 + NaOH+ NaHSO3 arrow K2MnO4 (green coloured-solution) + H2O + Na2SO4. If too much HSO3^- was added to this solution, what would be the resulting colour and why?
- In the gravimetric method, why is the reaction solution tested with litmus paper?
- 1. what is the smell and odor of NaCl when you add AgNO 3 and HNO 3 . 2. What is the smell and odor of NaBr when you add AgNO 3 and HNO 3 . Does a precipitate form? 3. What is the smell and odor o
- After a reaction involving copper (II) sulfate (blue) and aluminum metal are involved, there is a tinge of blue solution. The blue solution indicates: a) excess CuSO4 b) limited amounts of Al2(SO4)3 c) excess Al2(SO4)3 d) limited amounts of CuSO4
- Frequently, you can determine that a reaction is occurring when you observe precipitation. Precipitation, in this case, means: a) it is raining outside. b) a gas is evolving and you see bubbles. c) the color is changing. d) a solid is forming. e) it is sn
- what initially forms as pale blue and pale green precipitates when NH₃(aq)is added to (Cu solution (H₂ O)₆)²⁺ and ( Ni(H₂ O)₆)²⁺ solutions respectiv
- The aqueous solution of copper sulphate & zinc sulphate appear how?
- A student measures the potential of a cell made up with 1.0M CuSo4 in one solution and 1.0M AgNO3 in th other. There is a Cu electrode in the CuSO_4 and a Ag electrode in the AgNO_3. A salt bridge con
- How would the observed timing for precipitate formation change if 2-chlorobutane was subjected to silver nitrate in 1:1 ethanol:water (as opposed to 100% ethanol) ?
- A student was assigned a colorless unknown. The student added five drops of 1.0 M barium chloride solution to 1.0 mL of the unknown solution. A white precipitate formed. In a second experiment, the student added two drops of 0.5 M NH3 solution to 1.0 mL o
- 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
- a. State specifically how you would make a conclusive test for an iron (III) salt. b. Which test for iron (II) ions is conclusive. c. Suppose you have a solution containing both an iron (II) salt and an iron (III) salt. How would you proceed to identify
- Predict the outcome of storing a solution of CuSO4 in a container made of tin?
- If you put pure zinc metal into a solution of copper (II) sulfate, the zinc will slowly dissolve to produce a zinc sulfate solution, and the copper (II) ion of the copper (II) sulfate will be converte
- An unknown sample does not react with 2,4-dinitrophenylhydrazine reagent, but a color change is observed on reaction with ceric nitrate reagent.
- Copper sulfate is a hydrated crystal with the formula CuSO_4 cdot 5H_2O and a deep blue colour. When it's heated, the crystals crumble and turn white. (a) Propose an explanation for this change of c
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o When the sample coming off the ion exchange column has been collected, where are the colored ions?
- What would likely happen if you were to touch a metallic beaker in which an endothermic reaction were occurring? (A) The beaker would probably feel cooler than before the reaction started. (B) The bea
- (a) A student adds sodium bromide solution (NaBr) to a sample of the blue equilibrium mixture in order to increase the Br- ion concentration. Predict what the student will observe and explain the pred
- TestubeA: KMnO_4 + H_2SO_4 + NaHSO_3 \to MnSO_4 + K_2SO_4 + Na_2SO_4 (colourless solution) If test tube A wasn't acidic enough, what color might you expect in the products?
- Small pieces of silver, copper, and magnesium are placed in solutions that contain one of the following ions: Ag^+ Cu^2+ and Mg^2+. The metal/solution combinations tested are summarized in the followi
- Data Table 1. Redox Reaction of Copper and Silver Nitrate. Initial observations: before beginning Copper: thin squares Silver Nitrate: Clear Liquid Observations Cu turning black Observations after
- The test solution is made basic and drops of .1 M Ca(NO3)2 are added but not precipitate forms. To what part of the experimental procedure do you proceed? Explain
- 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
- Determine which liquid is which, two blue solutions and two clear choices: CuSO4 Cu(NO3)2 NH4OH CaCl2
- Through the solution of the sulfate of the unknown divalent metal, the current I = 0.5 A was in a time t. The volume of resulting metal is 1.5 mL. It was discovered that this metal crystallized by the type of face centered cube with a = 352 pm. How long
Explore our homework questions and answers library
Browse
by subject