In your own words, Explain What is an indicator? Does it have a significant value in chemical reaction? Give an examples of indicators and their uses.
Q: When the following solutions are mixed together, what precipitate (if any) will form? Note: Leave…
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Q: You have been asked to determine the concentration of a dilute HCl solution. What method will be…
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Q: Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used…
A:
Q: What are the solubility rules? How are they useful?
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Q: Define and give an example of each of the following classes of reactions: precipitation, acid–base,…
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Q: On the basis of the general solubility rules, predict which of the following substances are likely…
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Q: Write a net ionic equation to show that hydrofluoric acid, HF, behaves as an acid in water
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Q: Calculate the molarity of an acetic acid (FW 60,052) solution if 25 mL of this solution is…
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Q: نقطتان )2( the Gravimetric analysis can ----:consider as The quantitative methods that are based on…
A: Gravimetric analysis:
Q: Complete and balance the precipitation reactions. Include physical states. Refer to the solubility…
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Q: Using the general solubility rules, predict the following substances as soluble or insoluble in…
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Q: write the ionic and net ionic equations. 1.) ___ H3PO4 + ___ NaOH -> ionic equation: net ionic…
A: 1.) ___ H3PO4 + ___ NaOH -> 2.) ___ HI + ___ LiOH -> 3.) ___ HNO3 + ___ Ca(OH)2 ->…
Q: Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used…
A: Reaction occurHCl(aq) + NaHCO3(aq) → NaCl(aq) + CO2(g) + H2O(l)Molarity of HCl = 0.078 MVolume…
Q: Balance the following reaction, and using the given solubility table as reference write (s)/(aq)…
A: A balanced equation is an equation in which the number of atoms for each element in the reaction…
Q: Sodium hydrogen carbonate (NaHCO,, also known as sodium bicarbonate or "baking soda", can be used to…
A: Given, HCl(aq) + NaHCO3(aq) ➝ NaCl(aq) + H2O(l) + CO2(g) Molarity of HCl solution = 0.040 M = 0.040…
Q: solution of potassium carbonate is prepared in water, then hydrobromic acid is added dropwise. 2)…
A: Balancing chemical equations.
Q: Which of the following will occur when solutions of Na,SO (aq) and CaCl,(aq) are mixed? I. A…
A: Given that the solution of Na2SO4 and CaCl2 are mixed.
Q: Include states of matter in your balanced equation. Write a balanced net ionic equation for a…
A: When acid and a base react with each other to form salt and water. This reaction is well known as…
Q: For the chemical reaction HCN(aq)+KOH(aq)⟶H2O(l)+KCN(aq)HCN(aq)+KOH(aq)⟶H2O(l)+KCN(aq) write…
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Q: KBr AgNO3 Ej: KBr + AgNO3 →→KNO3 AgBr Na2CO3 Cas NHẠCH
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Q: For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction…
A: Gravimetric analysis is a method of quantitative chemical analysis in which the constituent is…
Q: On the basis of the general solubility rules given in table 4.1 predict which of the following…
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Q: The reaction between hydrochloric acid and sodium carbonate is represented by the equation 2HCI(ag)…
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Q: KI (aq) + AgNO3 (aq) --> AgI (s) + KNO3 (aq) Determine if a solid precipitate is formed in this…
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Q: 1a) complete the balanced overall ionic equation for the mixing of these two solutions. 2Na+(aq) +…
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Q: What is the balanced net ionic equation?
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Q: 2.0 M Mg(NO3)2(aq) is mixed with 2.0 M NaF(aq). Will a precipitate form upon the mixing of these two…
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Q: A student is given the following labeled solutions: NaCl, The data was collected and summarized in…
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Q: Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used…
A:
Q: Sodium hydrogen carbonate (NAHCO,), also known as sodium bicarbonate or "baking soda", can be used…
A: Given, NaHCO3 neutralizes excess HCl through the reaction, HCl (aq) + NaHCO3 (aq)…
Q: Complete and balance the precipitation reactions. Include physical states. Refer to the solubility…
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Q: A. Write a balanced chemical equation, total ionic equation and net ionic equation for the given…
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Q: 1. Complete and balance the following neutralization equations. H2SO4 + NaOH -> __ +__ ____+_____…
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Q: On the basis of the general solubility rules, predict which of the following substances are likely…
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Q: Define and give an example of each of the following classes of reactions: precipitation, acid–base,…
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In your own words, Explain What is an indicator? Does it have a significant value in
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- A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H+ or OH ions left in solution.The procedures and principles of qualitative analysis are coy cred in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.Write the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.
- 42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.Consider the following generic equation OH(aq)+HB(aq) B(aq)+H2OFor which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) hydrochloric acid and pyridine, C5H5N (b) sulfuric acid and rubidium hydroxide (c) potassium hydroxide and hydrofluoric acid (d) ammonia and hydriodic acid (e) strontium hydroxide and hydrocyanic acid
- Many plants are poisonous because their stems and leaves contain oxalic acid H2C2O4, or sodium oxalate, Na2C2O4. When ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, C2O42 in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Write die net ionic equation for the reaction between sodium oxalate and calcium chloride. CaCl2, in aqueous solution.Describe some physical and chemical properties of acids and bases. What is meant by a strong acid or base? Are strong acids and bases also strong electrolytes? Give several examples of strong acids and strong bases.Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
- The Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b From everyday experience you are probably aware that table sugar (sucrose), C12H22O11, is soluble in water. When sucrose dissolves in water, it doesnt form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water. c Both NH3 and C12H22O11 are soluble molecular compounds, yet they behave differently in aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte. d Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water. e Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes? f Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte. g Classify each of the following substances as either ionic or molecular. KCl NH3 CO2 MgBr2 HCl Ca(OH)2 PbS HC2H3O2 h For those compounds above that you classified as ionic, use the solubility rules to determine which are soluble. i The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water. j Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water? k How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer. l Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m Are NaCl and HI strong electrolytes because they have similar behavior in aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case. Part 2: You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water. AX(aq)+H2O(l)AH2O+(aq)+X(aq)AY(aq)+H2O(l)AH2O+(aq)+Y(aq) a Explain how the relative amounts of AX(aq) and AY(aq) would compare if you had a beaker of water with AX and a beaker of water with AY. b How would the relative amounts of X(aq) and Y(aq) in the two beakers compare? Be sure to explain your answer.hat kind of visual evidence indicates that a chemical reaction has occurred? Give an example of each type of evidence you have mentioned. Do all reactions produce visual evidence that they have taken place?Equal quantities of the hypothetical strong acid HX, weak acid HA, and weak base BZ are added to separate beakers of water, producing the solutions depicted in the drawings. In the drawings, the relative amounts of each substance present in the solution (neglecting the water) are shown. Identify the acid or base that was used to produce each of the solutions (HX, HA, or BZ).