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For each of the following water-soluble compounds, indicate the ions present in an aqueous solution: NaI K2SO4 NaCN Ba(OH)2 (NH4)2SO4 would the answer to NaI be Na+ I-? Should there be more to my answer? Would K2SO4 be K+ SO-?

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  1. Chem answer check/ help

    For each of the following water-soluble compounds, indicate the ions present in an aqueous solution: NaI K2SO4 NaCN Ba(OH)2 (NH4)2SO4 would the answer to NaI be Na+ I-? Should there be more to my answer? Would K2SO4 be K+ SO-? Thanks for the explanation.

  2. Chemistry

    1. Give one possible error you could have made in carrying out the experiment (not a calculation error) that would cause your. a) %NaCl to be too small b) %SiO2 to be too large 2. Solubilities of Compounds A, B and C were determined and summarized in the

  3. CHEMISTRY

    list three differences between molecular and ionic compounds, and explain how they relate to the differences in bond types.....how do i relate to the differences in bond types? List the differences and we'll talk about how they relate to the bond type. 1.

  5. science(chem)

    Solubility: Solubility of compounds in a)water (highly polar) b)methyl alchohol (intermediate polarity) c)Hexane (nonpolar) My guess 1. Benzophenone a) not soluble b) partially soluble c) soluble 2. Malonic acid a) soluble (since it's polar) b) soluble c)

  6. chemistry

    which of the following liquids have the highest freezing point? a- aqueous Fe(NO3)3 (0.030) b- aqueous glucose (0.050 m) c- aqueous NaI (0.030 m) d- aqueous NaI (0.010 m) e- pure water please explain the concept behind it as well thank you!

  7. chemistry

    what evidence supports the clarification that H2Se 03 is an acid and how do i identify the positive ions present inthe aqueous solution I am a little confused by the word "clarification" in your question. What evidence do you have? Could you measure the pH

  8. chem

    A solution is prepared by dissolving 0.87mol of MgCl 2 in 0.40kg of water. How many moles of ions are present in solution? What is the change in the boiling point of the aqueous solution?

  10. chemistry

    1. 2IO3- + 10Ag+ 12H+I2 + 10Ag++ 6H2O In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. 2. Write a net ionic equation for the reaction that occurs when

  11. Chemistry

    Some amount of water is evaporated from a 2.0 L, 0.2 M NaI solution, to from a 1.0 L solution. The molar mass of NaI is 150 g/mol. What is the final concentration of NaI solution in?

  12. Science

    Some amount of water is evaporated from a 2.0 L, 0.2 M NaI solution, to from a 1.0 L solution. The molar mass of NaI is 150 g/mol. What is the final concentration of NaI solution in? A. 30 g/L B. 15 g/L C. 60 g/L D. 45 g/L

  13. chemistry

    An aqueous solution is analyzed and found to contain potassium ions and sulfite ions. Write the equation for the dissolution of the salt that produced this solution. If the solution contains 0.600 mol of potassium ions, how many moles of sulfite ions are

  15. AP Chemistry

    Consider the following reaction: PbCl2 + 2 NaOH → Pb(OH)2 + 2 NaCl What would be the major species observed floating in solution after one mole of PbCl2 and 2 moles of NaOH are mixed in aqueous solution? 1. Na+ ions, Cl− ions and H+ ions 2. Pb2+ ions,

  16. Chemistry

    Consider the following reaction: PbCl2 + 2 NaOH -> Pb(OH)2 + 2 NaCl What would be the major species observed floating in solution after one mole of PbCl2 and 2 moles of NaOH are mixed in aqueous solution? 1. Na+ ions, Cl− ions and H+ ions 2. Pb2+ ions,

  17. Chemistry

    Please help me....are these questions right or no? If not can you help me...any suggestions please? 7.(14). Which of the following is a salt? a. HNO3 b. H2SO4 c. CaSO4 d. NaOH e. NH3 I put down C- CaSO4, is that right or am I way off track? 8.(15). Which

  18. Science

    Ionic compounds dissolve in water, and their ions separate from each other. If a sample of Al2S3 containing 16 aluminum ions is dissolved in water, how many sulfide ions will be present? So, two cations and three anions. Would we have one sulfide ion left?

  20. chemistry

    I have two Questions I need help with. 1. Why do some combinations of ionic compounds form a precipitate while other ionic compounds don't? AND 2. Solutions of lead(II)nitrate and potassium iodide are combined in a test tube and form a yellow precipitate.

  21. Chemistry

    What makes the strongest cation in water? Al Na Fe K Mg I know that the OH^- ions from water are enough for the Al(OH)3 and Fe(OH)3 precipitates to appear and we've been taught that K,Na compounds are soluble in water too. And Mg(OH)2 needs a higher OH^-

  22. chemistry

    If 740. mL of 0.06622 M aqueous NaI and 370. mL of 0.07151 M aqueous Pb(NO3)2 are reacted stoichiometrically according to the equation, what mass (g) of NaI remained? Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)

  23. college chemistry

    1) If 740. mL of 0.06622 M aqueous NaI and 370. mL of 0.07151 M aqueous Pb(NO3)2 are reacted stoichiometrically according to the equation, what mass (g) of NaI remained? Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq) 2) If 180 mL of 0.581 M aqueous HCl

  25. Chemistry

    Decide whether each of the following is water-soluble. If soluble tell what ions are produced. A. Na2CO3 B. CuSO4 C.NiS D.BaBr2 I put soluble for A, B, and D. But i can not figure out the ions that are produced??

  26. chemistry

    1. Divide the ions below into 2 groups, those that tend to form soluble compounds and those that tend to form insoluble compounds. (〖Pb〗^(+2), 〖Na〗^+, 〖Nh4〗^+, 〖Ag〗^+, 〖NO3〗^-, 〖OH〗^-, 〖Cl〗^-, 〖CO3〗^(-2), 〖PO4〗^(-3)) 2.

  27. Chemistry - solubility

    Arrange the following compounds in order of increasing solubility in water: * O2 * LiCl * Br2 * CH3OH Like dissolves like; that is, polar compounds usually are soluble in water and non-polar compounds are not soluble in water. From that description, make

  28. chemistry

    Water softeners often replace calcium ions in hard water with sodium ions. Since sodium compounds are soluble, the presence of sodium ions in water does not cause the white, scaly residues caused by calcium ions. However, calcium is more beneficial to

  30. Chemistry

    Explain Why some ionic compounds are soluble in water. Explain why non-ionic compounds, such as ethanol or sugar are soluble in water. Explain what a saturated solution.

  31. Chemistry

    Which argument supports the claim that dissolving solid calcium chloride (CaCl2) in water is a chemical change? A. The ionic bond between the calcium ions and chloride ions is broken. B. The solid calcium chloride can be recovered by evaporating the water.

  32. Chemistry

    i was wondering which ones are soluble in water and what ones are not: K2CrO4, CaS, Na2S, and BaSO4 I was also wondering if AgBr and CaCO3 are soluble as well. BaSO4, AgBr and CaCO3 are insoluble. The others are soluble. I can give you a web site that

  33. Chemistry (CHEM)

    Can someone explain the electrical conductivity of melted and of aqueous solutions of ionic compounds. An explain it using the characteristics of ionic compounds. ThankS A Whole lot.. In Advance I suggest you go to the site recommended by Ms.Sue. Here is a

  35. science

    When salt (NaCI) is added to water, it disassociates into Na and Cl-ions. Which of the following types of chemical bond is present in a salt molecule? A. Covalent bond B. Ionic bond C. Hydrogen bond D. Disulfide bond i think its B An example of active

  36. College Chem 1

    a chemistry handbook lists the solubility of NaI as 184 per 100mL of H2O at 25 degrees Celcius. 1) How many moles of NaI can be dissolved in 100mL of H2O at 25 degrees Celcius? 2) What would be the molarity of a saturated aqueous solution of NaI prepared

  37. Chemistry

    When asked to name all of the ions and molecules present in a 0.1 mol L-1 solution of CH3COOH, why are there OH- ions present if the equation is CH3COOH(aq) + H2O(l) --> CH3COO-(aq) + H3O+(aq) ? The water ionizes in such a manner that the product of the

  38. chemistry

    Okay so the question is: what would be the molarity of a saturated aqueous solution of NaI prepared at 25 C, assuming that the added NaI does not add significantly to the volume of the water? My question is, I got confused on what formula I use to for the

  40. Chemistry

    Consider the strengths of the following changes: separate NaI into its ions: 702 kJ/mol separate water into molecules 60 kJ/mol form solvent shells around sodium ions and iodide ions 770 kJ/mol When dissolving NaI in water, the change is likely to be

  41. Chemistry

    Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12× 10–12. What is the solubility (in mol/L) of silver chromate in 1.4 M potassium chromate aqueous solution? In 1.4 M silver nitrate aqueous solution? In pure water?

  42. Chemistry II - Concentrations

    At 30.°C, the concentration of hydronium (H3O^+) ions in an aqueous solution is 1.1 ✕ 10^−9 M. (Note: At 30.°C, the ion-product constant for water is 1.46 ✕ 10^−14.) (a) What is the concentration of hydroxide (OH^−) ions in this solution? (b)is

  43. Chem

    A compound that dissolves in water to form an aqueous solution that is an excellent conductor of electricity is always present in the solution as -covalent molecules -acid molecule -base molecule -salt molecules -ions

  45. Organic Chemistry

    Why is 4-chlorophenol soluble in 2.5M NaOH solution, but not in water? A. Phenol is a weak acid so it can be deprotonated under basic conditions. B. Aqueous acid destroys 4-chlorophenol. C. 4-chlorophenol is only soluble in water at low temperature. D. A

  46. chemistry

    What is a special group of compounds that produce H+ ions when dissolved in water? A. Acids B. Ionic compounds C. Molecular compounds D. Polyatomic compounds I think A

  47. chemistry

    copper compounds such as copper (II) sulfate are toxic. before disposal, these compounds must be treated to reduce their toxicity. describe how to use steel wool to remove the Cu 2+ ions from an aqueous solution of copper (II) sulfate

  48. Chemistry

    What volume of each solution contains 0.220mol of NaI? a.) 0.142M NaI b.) 0.902M NaI c.) 1.61M NaI

  50. Aqueous Solution

    Write the positive and negative ions that result when the following compounds are dissolved in aqueous solution: Na2S (aq): (NH4)2CO3 (aq): K2SO4 (aq):

  51. aqueous solution

    Write the positive and negative ions that result when the following compounds are dissolved in aqueous solution: Na2S (aq): (NH4)2CO3 (aq): K2SO4 (aq):

  52. chemistry

    Excess aqueous NaI was added to 50 mL of aqueous CuNO3 solution, and 28.72 g of CuI precipitate was formed. What was the molar concentration of CuNO3 in the original solution? Answer in units of M.

  53. Chem

    If 390 mL of 0.0410 M aqueous NaI(aq) and 1.36 g of liquid Br2 are reacted stoichiometrically according to the equation, what mass (g) of NaI(aq) remained? 2 NaI(aq) + Br2(l) �¨ 2 NaBr(aq) + I2(s) Molar Mass (g) NaI(aq) 149.89 Br2 159.81 Molar Volume (L)

  55. Chemistry I'm in dire need of of assistance!!!

    Which statement best describes what it means when something is classified as a strong acid?(1 point) 1. it resists dissociating into ions in solution 2. It is present in large quantities in a solution 3. It easily dissociates into ions in solution 4. It is

  56. Chemistry

    A 500.0-mL sodium iodide (NaI) solution was prepared by dissolving 37.7g of solid NaI in water. Chlorine gas was bubbled through a 100.0-mL sample of this solution until the reaction was complete. How many grams of molecular iodine were produced?

  57. Chemisty

    Before solving the problem write a balanced chemical equation Excess aqueous NaI was added to 50 mL of aqueous CuNO3 solution, and 14.2 g of CuI precipitate was formed. What was the molar concentration of CuNO3 in the original solution? Answer in units of

  58. Chemical Formulas and Reactions

    When aqueous copper(II)chloride reacts with aqueous ammonium phosphate, soluble ammonium chloride forms and copper(II) phosphate precipitates out of solution. 1. Write the balanced molecular equationfor this reaction. 2. Write the balanced complete ionic

  60. Chemistry

    Which of the compounds is more soluble in an acidic solution than in pure water? a. PbBr2 b. CaS c. Zn(OH)2 d. BaSO3 e. RbClO4

  61. Chemistry

    How many number of ions of each type are present in the following aqueous solution? 113 mL of .490 M aluminum chloride.

  62. Organic Chemistry

    Does Ethanoyl Chloride gives out a white precipitate with aqueous AgNO3? We've been thought that an acid chloride gives out the relative Carboxylic acid with water.So in the same way can we take that Ethanoyl Chloride reacts with the water in this aqueous

  63. chemistry

    Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases. What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.350 L of 0.290 M NaI? Assume the reaction goes to completion.

  65. Chemistry

    How many moles and number of ions of each type are present in the following aqueous solution? 113 mL of .490 M aluminum chloride.

  66. Chemistry

    2. The reaction can be described in words as follows: aluminum sulfate reacted with ammonium hydroxide forming the insoluble product or precipitate, aluminum hydroxide and the water-soluble ammonium sulfate. The chemical equation can be written as follows

  67. Easy chem question... me=braindead, help please?

    It's been so long I forget which ones are which. My balanced equation is Sr(NO3)2 + 2KIO3 --> Sr(IO3)2 + 2KNO3. It wants the total ionic and the net ionic Thanks ^^ (not just looking for answer, want explanation too please, just a short one) In aqueous

  68. Chemistry

    A concept map was to be created on acids and bases. The concept terms that were given to use were: aqueous solution,bases,acids,ions,weak bases, strong bases, strong acids, weak acids,dissociation, weak electrolyte, strong electrolyte,reaction,salt,

  70. aP Chemistry

    The net ionic equation for ALL aqueous reac- tion of strong acids and strong soluble bases that form soluble salts is 1. the formation of the soluble salt. 2. the formation of water from the ele- ments. 3. the formation of H2O from H and OH . 4. the

  71. Chemistry

    A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 Celsius. Assuming that the organic

  72. ap

    The net ionic equation for ALL aqueous reac-tion of strong acids and strong soluble bases that form soluble salts is 1. the formation of H2O from H+ and OH−. 2. the formation of water and the corresponding salt. 3. the formation of water from the

  73. SCIENCE

    (aq) means the solution is dissolved in water used as a solvent. (l) means the COMPOUND (not element, usually) is a pure liquid. (g) means gas and (s) means solid. In the equation below, HCl(aq) + NaOH(aq) -->NaCl(aq) + H2O(l)This means that an aqueous

  75. Chemistry check

    First, percent error can be negative, correct? Because in my lab I got -32%. Here are my questions that I need checked: 1. List possible manipulation errors that might contribute to the following errors in results: 1) obtaining a significantly larger

  76. Science --HELP PLEASE

    I need to write a hypothesis for a lab ex. I think that ionic compounds will be soluble in water because the polar molecules in H20 cause the compound to break apart and dissolve in the water. but another part is the appearance of ionic and covalent

  77. chemistry

    Which solution would CaC2O4 be most soluble in? Na2C2O4 NaHC2O4 H2C2O4 NaCl HCl I due to common ions i think it would be one of the first three and i think it is Na2C2O4 because the other 2 have Hydrogen. Is it Na2C2O4? No, the common ions work just the

  78. chem

    what would the equation for this reaction be?; KAL(SO4)2.12H2O crystallizes out when water is cooled enough to cause the soluble ions to coalesce and precipitate out of solution.

  80. Chemistry

    If a solution has a total mass of 26.7g and is 8.36 % by weight in sodium chloride, what mass of sodium chloride is present in the solution? How many moles of dextrose (C6H12O6) are in 414mL of solution with a concentration of 0.84M? If an aqueous solution

  81. chemistry

    Please I need help. Many,but not all, compounds are made up of positive and negative ions. Three positive ions A^+, B^2+ and C^3+ could form a total of six different compounds with negative ions, Y^2- and Z^3-. Derive the formulae for six compounds and

  82. Chem I

    Are there any tricks for remembering solubility rules? I am having a hard time remembering which compounds are soluble and which are not. Any suggestions would be appreciated, I just get the soluble/insoluble compounds mixed up sometimes.

  83. Chemistry

    Is PbI2 soluble in water or not? Following the solubility rules for ionic compounds, salts containing Pb are insoluble and iodide salts are soluble, so can it be both?

  85. chemistry.

    When 41.81 of a solution of aqueous sliver ions with a concentration of 0.2040 mol dm3 is added to a solution of XO-3/4 ions, 1.172g of the precipitate is formed? ..Can any one help me with that! NB: -3/4 mean that 3 is up and 4 is under it.

  86. chemistry(rusting)

    Why metal(eg. iron)placed at aqueous solution will be more easily occur rusting?Is it due to the mobile ions in the aqueous solution ?Please give me an detail explanation ,thank you.

  87. science

    what are 4 differences between ionic and covalent bonding? plz help thanks!! http://antoine.frostburg.edu/chem/senese/101/compounds/faq/properties-ionic-vs-covalent.shtml i clicked on the link but it doesnt tell me anything See if it works (Broken Link

  88. Chemistry

    A solution is made by dissolving 1.0 mole of Na2SO4(ionic compound) into water to get 1.0L of solution. Give the conc of all the ions present in solution in M?

  90. Chemistry Plz hurrry

    What are charateristic of a ionic bond and a chemical bond? An ionic bond is a type of chemical bond that involves gain or loss of valence (outer shell) electrons in order to attain stability. That is not what I am looking for but thanks anyway An ionic

  91. chemistry

    Will you help me use the half reaction method to balance these equations. I need to add water molecules and hydrogen ions in acid solutions. I also need to keep the balanced equations in net ionic form. thanks 1) Cl-(aq) + NO3-(aq) --> ClO-(aq) +NO(g) (in

  92. chemistry

    Salts that are insoluble in water are made by precipitation. ● Lead(II) iodide, PbI2, is insoluble in water. ● All nitrates are soluble in water. ● All sodium salts are soluble in water. You are provided with solid lead(II) nitrate, Pb(NO3)2, and

  93. science

    Ions are electrically charged particles that are formed when certain compounds are dissolved in water. These solutions will conduct electricity. The Swedish scientist Svante Arrhenius coined the term ion (which means wanderer) to explain why solutions of

  95. Science

    Ions are electrically charged particles that are formed when certain compounds are dissolved in water. These solutions will conduct electricity. The Swedish scientist Svante Arrhenius coined the term ion (which means wanderer) to explain why solutions of

  96. Science

    Ions are electrically charged particles that are formed when certain compounds are dissolved in water. These solutions will conduct electricity. The Swedish scientist Svante Arrhenius coined the term ion (which means wanderer) to explain why solutions of

  97. Chemistry

    In concentrated aqueous solutions of NaCl, the Na+ (aq) ions can be so close to the Cl- (aq) ions that a small percentage is associated in ion pairs at any given moment. Suppose that a solution contains 1.00 mol of NaCl and that 5.57% of the formula units

  98. Chem

    According to the Arrhenius Theory of acids and bases, a base is: A A substance that decrease the amount of hydroxide ions present. B A substance that increases the amount of hydroxide ions present when it is dissolved in water. C A substance that increase

  100. Chemistry 12

    15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is: a. 2 x 10-14 M b. 5 x 10-14 M c. 5 x 10-7 M d. 2 x 10-1 M 16. Aqueous solutions of strong acids and strong bases: a. are good electricity conductors b. make litmus paper become

  101. science

    Ions are electrically charged particles that are formed when certain compounds are dissolved in water. These solutions will conduct electricity. The Swedish scientist Svante Arrhenius coined the term ion (which means wanderer) to explain why solutions of

  102. Science

    Ions are electrically charged particles that are formed when certain compounds are dissolved in water. These solutions will conduct electricity. The Swedish scientist Svante Arrhenius coined the term ion (which means wanderer) to explain why solutions of

  103. Science

    5. You have made the following two solutions: X) hydrogen ion concentration = 1 x 10-5M Y) pH = 4 State which statements below are true and which are false: a. Solution X contains 1 x 10-9M hydroxide ions. b. Solution X contains more H+ ions than Solution

  105. chemistry

    The density of a 2.45 M aqueous methanol solution is .976 g/ml. what is the mass of water present in 1.00 liter of this solution

  106. chemistry

    What are the certain conditions when ionic compounds conduct an electric current? Why are ionic compounds not always used as conductors? Ionic compounds conduct an electric current when the ions are free to move about. This usally means they are in

  107. Chemistry

    I was asked to consider the solubility for hydrated calcium sulfate in HCl. The principal acid my proffesor had posted for the solution was [ CaSO4(hyrdrated) + HCl H30^+ + Ca^2+ + SO4^2- ]. I guess what I'm asking is what happened to the Cl^- and why

  108. Chemistry

    What is the charatteristic of covalent bonding meaining what happens and then what is the result from what happened (like does it form a molecule, compund, etc. . . Same thing for ionic bodnging The ionic part is discussed below. Look for a chemistry post

  110. Chemistry

    The net ionic equation for ALL aqueous reaction of strong acids and strong soluble bases that form soluble salts is 1. the formation of H2O from H+ and OH−. 2. the formation of water from the ele-ments. 3. the formation of water and the corre-

  111. Biology

    1)Which of the following is NOT a true property of water? A-Water is a good solvent dissolving a wide variety of substances. B-Water has a high ice density allowing ice to sink when present with liquid water. C-Water has strong cohesion allowing it to bead

  112. Chemistry

    When hypochlorite ions act as an oxidizing agent, hydroxide ions are formed. What will this do to iron (II) or to iron (III) ions? Both Fe(OH)2 and Fe(OH)3 are insoluble in an aqueous solution.

  113. Chemistry

    A salt was completely soluble in water. When this solution was treated with AgNO3 no precipitate was formed. What anions could be present?

  115. chemistry

    Ions in aqueous solution that are surrounded by polar water molecules are said to be saturated. is it true or false?

  116. Chemistry

    How many (a) H+ ions (1 g-ion/L = 6.023 x 1023 ions/L) and (b) OH- ions are present in 250 ml of a solution of pH 3?

  117. Biochemistry

    How many a) H+ ions (1 g-ion/L = 6.023 x 1023 ions/L) and b) OH- ions are present in 250 ml of a solution of pH 3?

  118. chemistry

    The compound sodium sulfate is soluble in water. When this compound dissolves in water, which ion listed below would be present in solution?

  120. Chemistry

    My question is basically to find out what these reactants yield: CuCl2(aq) + NH3(aq) --> ? my best guess here is... CuCl2(aq) + 6NH3(aq)-->[Cu(NH3)4(H2O)2]2+ + N2(g) + 2HCl Im pretty sure about the [Cu(NH3)4(H2O)2]+2 part but not sure about the rest. The

  121. 10th grade chemistry

    We're doing a lab report on the hardness of water, and one of the calculations is "The EDTA reacts with the hard water ions in a 1:1 mole ratio. Calculate the molarity of the ions present in 20 mL of water tested." How would you do this?

  122. chemistry

    Which of the following statements about boiling points are true? A. The boiling point of 0.1 m NaF(aq) is lower than the boiling point of 0.1 m methanol(aq). B. The boiling point of a 0.5 m aqueous solution of LiOH is the same as the boiling point of a 0.5

  123. chemistry

    A solution contains 4.44% by mass of NaI in water. Calculate the molarity of the NaI, if the density of the solution is 1.2711 g mL-1. i got the answer to be 8.48 M... the percent mass is irrelevant information, right? i figured out the answer just by the

  125. Chemistry

    An aqueous solution of barium nitrate has a density of 1.09 g/cm3. The solution is 18.7% barium nitrate by mass. How many nitrate ions are present in 87.6 dL of this solution?

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