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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Consider the beaker below, which represents a saturated solution of AgCl(aq). Draw a picture of the solution in the beaker after the addition of NaCl(aq).
If you add a dilute acidic solution to a mixture containing magnesium oxalate and calcium oxalate, which of the two compounds is more likely to dissolve?
Suppose the molar solubility of nickel hydroxide, Ni(OH)2, is x M. Show that Ksp for nickel hydroxide equals 4x3.
A solution containing calcium ion and magnesium ion is buffered with ammonia-ammonium chloride. When carbonate ion is added to the solution, calcium carbonate precipitates but magnesium carbonate
A solution contains 0.00750 M calcium ion. A concentrated sodium fluoride solution is added to precipitate calcium fluoride (assume no volume change). a. At what concentration of F does precipitate
a. If the molar solubility of cobalt(II) hydroxide is 5.4 × 10–6 mol/L in pure water, what is its Ksp value?
a. If the molar solubility of beryllium(II) hydroxide is 8.6 × 10–7 M in pure water, what is its Ksp value?
Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia.a. What is the equilibrium constant for this dissolving process?
Crystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate.a. What is the equilibrium constant for this dissolving process?
A 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a. What is the hydroxide-ion concentration of this solution? b. 0.075 mol of MgCl2 is added to the above solution.
A 1.0-L solution that is 1.6 M in ammonia is mixed with 75.8 g of ammonium sulfate. a. What is the hydroxide-ion concentration of this solution? b. 0.058 mol of MnCl2 is added to the above solution.
What chemical reaction is responsible for the dissolving out of caverns in limestone caves?
What chemical reaction is responsible for the formation of stalactites and stalagmites in limestone caves? How is this reaction related to the one involved in the dissolving out of caverns?
You add 50.0 mL of 0.100 M HCl to 50.0 mL of 0.100 M AgNO3. What are the final concentrations of H3O+ and Cl in the solution?
A chemist mixes 1.00 L each of 0.100 M Na2CO3 and 0.200 MCaCl2 in a beaker. What is the concentration of carbonate ion, CO32, in the final solution?
A researcher found the solubility of lead(II) bromide in 0.100 M NaBr to be 1.31 g/L. What is the solubility product of lead(II) bromide?
Gout is a painful inflammation of the joints caused by an excess of uric acid in the blood and its precipitation as sodium urate (the sodium salt of uric acid), NaC5H3N4O3, in tissues of the joints.
An analytical chemist has a solution containing chloride ion, Cl-. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 MAgNO3. As a way
How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride?
A scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is
A 1.00-g sample of solid barium sulfate and a similar 1.00-g sample of solid calcium sulfate were added to water at 25°C to give 1.00 L of solution. Calculate the concentrations of Ba2+, Ca2+, and
Calcium fluoride, CaF2, is a very slightly soluble salt. In Example 17.4, we calculated its solubility from the solubility constant, assuming that the solubility equilibrium represented by Ksp was
You slowly add ammonia, NH3, to 1.00 L of water containing 5.00 g of solid nickel(II) iodate, Ni(IO3)2. How much ammonia (in moles) would you have to add to just dissolve the nickel(II) iodate? What
A solution is 1.5 × 10-4 M Zn2+ and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is
A solution is 1.8 × 10-4 M Co2+ and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of cobalt(II) sulfide when the
What is the solubility of calcium fluoride in a buffer solution containing 0.45 M HCHO2 (formic acid) and 0.20 M NaCHO2? (Consider the equation CaF2(s) + 2H+(aq) ⇌ Ca2+(aq) + 2HF(aq), and solve the
What is the solubility of magnesium fluoride in a buffer solution containing 0.45 M HC2H3O2 (acetic acid) and 0.20 M NaC2H3O2? The Ksp for magnesium fluoride is 6.5 × 10-9. (Consider the equation
A 67.0-mL sample of 0.350 M MgSO4 is added to 45.0 mL of 0.250 M Ba(OH)2. What is the net ionic equation for the reaction that occurs? What are the concentrations of ions in the mixture at
A 50.0-mL sample of 0.0150 M Ag2SO4 is added to 25.0 mL of 0.0100 M PbCl2. What is the net ionic equation for the reaction that occurs? What are the concentrations of ions in the mixture at
You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume
Consider three hypothetical ionic solids: AX, AX2, and AX3 (each X forms X). Each of these solids has the same Ksp value, 5.5 ×10–7. You place 0.25 mol of each compound in a separate container
Which compound in each of the following pairs of compounds is the more soluble one?a. Silver chloride or silver iodideb. Magnesium hydroxide or copper(II) hydroxide
You are given two mineral samples: halite, which is NaCl, and fluorite, which is CaF2. Describe a simple test you could use to discover which mineral is fluorite.
Explain why calcium sulfate is less soluble in sodium sulfate solution than in pure water.
Which of the following pictures best represents a solution made by adding 10 g of silver chloride, AgCl, to a liter of water? In these pictures, the gray spheres represent Ag+ ions and the green
Which of the following pictures best represents an unsaturated solution of sodium chloride, NaCl? In these pictures, the dark gray spheres represent Na+ ions and the green spheres represent chloride
When ammonia is first added to a solution of copper(II) nitrate, a pale blue precipitate of copper(II) hydroxide forms. As more ammonia is added, however, this precipitate dissolves. Describe what is
You add dilute hydrochloric acid to a solution containing a metal ion. No precipitate forms. After the acidity is adjusted to 0.3 M hydronium ion, you bubble hydrogen sulfide into the solution. Again
Use the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. a. NaBr b. PbI2 c. BaCO3 d. (NH4)2SO4
Use the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. a. Ca(NO3)2 b. AgBr c. MgI2 d. PbSO4
Write solubility product expressions for the following compounds. a. Mg(OH)2 b. SrCO3 c. Ca3(AsO4)2 d. Fe(OH)3
Write solubility product expressions for the following compounds. a. Ba3(PO4)2 b. FePO4 c. PbI2 d. Ag2S
The solubility of silver bromate, AgBrO3, in water is 0.0072 g/L. Calculate Ksp.
What must be the concentration of silver ion in a solution that is in equilibrium with solid silver chloride and that is 0.10 M in Cl?
The solubility of magnesium oxalate, MgC2O4, in water is 0.0093 mol/L. Calculate Ksp.
Calculate the solubility product constant for copper(II) iodate, Cu(IO3)2. The solubility of copper(II) iodate in water is 0.13 g/100 mL.
The solubility of silver dichromate, Ag2Cr2O7, in water is 1.59 g/L. Calculate Ksp.
The pH of a saturated solution of magnesium hydroxide (milk of magnesia) was found to be 10.52. From this, find Ksp for magnesium hydroxide.
A solution saturated in calcium hydroxide (limewater) has a pH of 12.35. What is Ksp for calcium hydroxide?
Strontianite (strontium carbonate) is an important mineral of strontium. Calculate the solubility of strontium carbonate, SrCO3, from the solubility product constant (see Table 17.1).
Magnesite (magnesium carbonate, MgCO3) is a common magnesium mineral. From the solubility product constant (Table 17.1), find the solubility of magnesium carbonate in grams per liter of water.
What is the solubility of PbF2 in water? The Ksp for PbF2 is 2.7 × 10–8.
What is the solubility of MgF2 in water? The Ksp for MgF2 is 7.4 × 10–11.
What is the solubility (in grams per liter) of strontium sulfate, SrSO4, in 0.23 M sodium sulfate, Na2SO4? See Table 17.1.
Discuss briefly how you could predict whether a precipitate will form when solutions of lead nitrate and potassium iodide are mixed. What information do you need to have?
What is the solubility (in grams per liter) of lead(II) chromate, PbCrO4, in 0.13 M potassium chromate, K2CrO4? See Table 17.1.
The solubility of magnesium fluoride, MgF2, in water is 0.016 g/L. What is the solubility (in grams per liter) of magnesium fluoride in 0.020 M sodium fluoride, NaF?
The solubility of silver sulfate, Ag2SO4, in water has been determined to be 8.0 g/L. What is the solubility in 0.45 M sodium sulfate, Na2SO4?
What is the solubility (in grams per liter) of magnesium oxalate, MgC2O4, in 0.020 M sodium oxalate, Na2C2O4? Solve the equation exactly. See Table 17.1 for Ksp.
Calculate the molar solubility of strontium sulfate, SrSO4, in 0.0015 M sodium sulfate, Na2SO4. Solve the equation exactly. See Table 17.1 for Ksp.
From each of the following ion concentrations in a solution, predict whether a precipitate will form in the solution.a. [Ba2+] = 0.020 M, [F] = 0.015 Mb. [Pb2+] = 0.035 M, [Cl] = 0.15 M
From each of the following ion concentrations in a solution, predict whether a precipitate will form in the solution.a. [Sr2+] = 0.012 M, [CO32] = 0.0015 Mb. [Pb2+] = 0.0012 M, [Cl] = 0.041 M
Lead(II) chromate, PbCrO4, was used as a yellow paint pigment ("chrome yellow"). When a solution is prepared that is 5.0 × 10-4 M in lead ion, Pb2+, and 5.0 × 10-5 M in chromate ion, CrO42, would
Lead sulfate, PbSO4, was used as a white paint pigment. When a solution is prepared that is 5.0 × 10-4 M in lead ion, Pb2+, and 1.0 × 10-5 Min sulfate ion, SO42, would you expect some of the lead
The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0020 M MgSO4. Is a precipitate expected? Explain.
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
A 45-mL sample of 0.015 M calcium chloride, CaCl2, is added to 55 mL of 0.010 M sodium sulfate, Na2SO4. Is a precipitate expected? Explain.
A 45.0-mL sample of 0.0015 MBaCl2 was added to a beaker containing 75.0 mL of 0.0025 M KF. Will a precipitate form?
A 65.0-mL sample of 0.010 M Pb(NO3)2 was added to a beaker containing 40.0 mL of 0.035 MKCl. Will a precipitate form?
How many moles of calcium chloride, CaCl2, can be added to 1.5 L of 0.020 M potassium sulfate, K2SO4, before a precipitate is expected? Assume that the volume of the solution is not changed
Magnesium sulfate, MgSO4, is added to 456 mL of 0.040 M sodium hydroxide, NaOH, until a precipitate just forms. How many grams of magnesium sulfate were added? Assume that the volume of the solution
What is the I concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl and 0.015 M I?
What is the Cl concentration just as Ag2CrO4 begins to precipitate when 1.0 MAgNO3 is slowly added to a solution containing 0.015 M Cl and 0.015 M CrO42?
Write the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.
Write the net ionic equation in which the slightly soluble salt lead(II) carbonate, PbCO3, dissolves in dilute hydrochloric acid.
Which salt would you expect to dissolve more readily in acidic solution, barium sulfate or barium fluoride? Explain.
Explain how metal ions such as Pb2+ and Zn2+ are separated by precipitation with hydrogen sulfide.
Which salt would you expect to dissolve more readily in acidic solution, calcium phosphate, Ca3(PO4)2, or calcium sulfate, CaSO4? Explain.
Write the chemical equation for the formation of the Cu(CN)2 ion. Write the Kf expression.
Write the chemical equation for the formation of the Ni(NH3)62+ ion. Write the Kf expression.
Sufficient sodium cyanide, NaCN, was added to 0.015 M silver nitrate, AgNO3, to give a solution that was initially 0.100 M in cyanide ion, CN. What is the concentration of silver ion, Ag+, in this
The formation constant Kf for the complex ion Zn(OH)42 is 2.8 × 1015. What is the concentration of zinc ion, Zn2+, in a solution that is initially 0.20 M in Zn(OH)42?
Predict whether cadmium oxalate, CdC2O4, will precipitate from a solution that is 0.0020 M Cd(NO3)2, 0.010 M Na2C2O4, and 0.10 M NH3. Note that cadmium ion forms the Cd(NH3)42+ complex ion.
Predict whether nickel(II) hydroxide, Ni(OH)2, will precipitate from a solution that is 0.0020 M NiSO4, 0.010 M NaOH, and 0.10 M NH3. Note that nickel(II) ion forms the Ni(NH3)62+ complex ion.
What is the molar solubility of CdC2O4 in 0.10 M NH3?
What is the molar solubility of NiS in 0.10 M NH3?
Describe how you could separate the following mixture of metal ions: Cd2+, Pb2+, and Sr2+.
Lead chloride at first precipitates when sodium chloride is added to a solution of lead nitrate. Later, when the solution is made more concentrated in chloride ion, the precipitate dissolves. Explain
Describe how you could separate the following mixture of metal ions: Na+, Hg2+, and Ca2+.
A student dissolved a compound in water and added hydrochloric acid. No precipitate formed. Next she bubbled H2S into this solution, but again no precipitate formed. However, when she made the
A student was asked to identify a compound. In an effort to do so, he first dissolved the compound in water. He found that no precipitate formed when hydrochloric acid was added, but when H2S was
Lead(II) sulfate is often used as a test for lead(II) ion in qualitative analysis. Using the solubility product constant (Table 17.1), calculate the molar solubility of lead(II) sulfate in water.
Mercury(II) ion is often precipitated as mercury(II) sulfide in qualitative analysis. Using the solubility product constant (Table 17.1), calculate the molar solubility of mercury(II) sulfide in
Mercury(I) chloride, Hg2Cl2, is an unusual salt in that it dissolves to form Hg22+ and 2Cl. Use the solubility product constant (Table 17.1) to calculate the following:(a) The molar solubility of
Magnesium ammonium phosphate is an unusual salt in that it dissolves to form Mg2+, NH4+, and PO43 ions. Ksp for magnesium ammonium phosphate equals 2.5 × 10–13. Calculate: (a) Its molar
For cerium(III) hydroxide, Ce(OH)3, Ksp equals 2.0 × 10–20. Calculate: (a) Its molar solubility (recall that taking the square root twice gives the fourth root);
Copper(II) ferrocyanide, Cu2Fe(CN)6, dissolves to give Cu2+ and [Fe(CN)6]4 ions; Ksp for Cu2Fe(CN)6 equals 1.3 × 10–16. Calculate: (a) The molar solubility, and (b) The solubility in grams per
What is the solubility of magnesium hydroxide in a solution buffered at pH 8.80?
A precipitate forms when a small amount of sodium hydroxide is added to a solution of aluminum sulfate. This precipitate dissolves when more sodium hydroxide is added. Explain what is happening.
What is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.50? The equilibrium is Ag2O(s) + H2O(l) ⇌ 2Ag+(aq) + 2OH(aq); Kc = 2.0 × 10-8.

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