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- [Nonacid] Molecules Dissolve... Intact hmg H2O C12H22011(s) → C,2H22O11(aq) A2??4 Covalent chemical bonds! H2O CH5OH(s)→ Co Hs OH (aq) H2O (sand) SiO,(s)→ → Molecular nonacid solutes disperse to single molecules (_) ...but no further! Dissolved nonacid molecules stay wholeWrite a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of manganese(II) sulfate and ammonium carbonate are combined. Do not include states such as (s) or (aq). It is not necessarry for you to indicate which of the products is the precipitate.For each of the following balanced chemical reactions, identify the type of chemical reaction. If you need to review this concept, select here. Choose... 2 Na(s) + Cl,(g) 2 NaC((s) simple decomposition V simple formation complete combustion 4 PCI(g) + P,(s) + 10 Cl,(g) double replacement 3Cuso,(aq) + 2Fe(s) → Fe,(so,),(aq) + 3Cu single replacement AGNO,(aq) + NaCI(aq) → AgCl(s) + NaNO,(aq) double replacement + 2 C,H2o(g) + 13 02(g) - 8 CO,(g) + 10 H,0(g) complete combustion +
- What would 2:3 4:1 2:1 4:3 ( 3 Which of the following would not be considered evidence of a chemical reaction? O A new color appears. precipitate is formed. An odor is given off. O Reactant changes phase. Complete the missing number to balance the following reaction. Sno, + 2 H, - Sn + 4.b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00 M NaCl (aq) in an Erlenmeyer flask. Both the AGNO, (aq) solution and the NaCl(ag) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. Which of the following is the complete ionic equation for the reaction that occurs in the beaker? A Ag+ (ag) + Cl- (aq) → AgCl (s) B Na (aq) + NO3 (aq) → NANO3 (s) Ag (aq) + NO, (aq) + Na (aq) + Cl-(aq) → AgCl(s) + Na* (aq) + NO, (aq) NaCl(aq) + AGNO, (aq) Ag (s) + NANO, (aq)
- Which of the statements about precipitation reaction is correct? It is a method that can be used for ions that can be partially precipitated. End point can be determined when precipitation ceases. It is a reaction process that requires the formation of soluble substances. It is a method that results to the formation of colored compounds with indicators before equivalence point. What is the expected end point result for the Assay of Sodium Chloride in Sodium Lauryl Sulfate? Red precipitate Black precipitate White precipitate Blue precipitate Which compound is formed at the end point for the Assay of Sodium Chloride? Ferric Ammonium Thiocyanate Ferric Sulfate Ferric Ammonium Chromate Ferric Thiocyanate How many milligrams of sodium chloride (MW = 58.44 g/mol) is equivalent to 1 N Silver Nitrate? 58.44 mg 5.844 mg 0.05844 g 0.5844 mg What is it that purpose of adding nitrobenzene in the Assay of Sodium Chloride? It is used as a convenient alternative to filtration…One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate, Suppose an EPA chemist tests a 200 mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl,(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂),(ag) The chemist adds 21.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 3.3 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. e -12 D.P C PNormally, the amount of silver nitrate required to precipitate all of the chloride in the sample is found by a trial and error process. However, to speed up the experiment, assume a sample mass of 0.1431 g, and that sample contains approximately 55.0% chloride ion by mass. From these assumptions, calculate the volume of 0.100 M AgNO3(aq) that needs to be added to precipitate all of the chloride ion. Please answer in mL. (Note: You are calculating the exact amount required and not adding 5mL in excess. In the experiment, you'd be adding an additional 5mL in excess since the chloride value of the salt may exceed 55%. Pay attention to the sig. figs. in your calculation; keep three sig. figs. in the answer.)
- Define and give an example of each of the following classes of reactions: precipitation, acid–base, gas evolution, redox (noncombustion), and combustion. Each group member can do one, and then present his or her reaction to the group.7. Despite the fact that the solubility rules have the word "rules" in the title, there are several exceptions to each that don't make much sense. The instance above shows a two of them. Which new statement fits best? Nitrate and Alkali metal salts are always soluble, Nitrate and Alkali metal salts are always soluble, except for Lithium Carbonate and Lithium Phosphate. Nitrate and Alkali metal salts are always insoluble, OO OHow much water (in mL) should you add to 50.0 mL of 0.300 M H,SO, (ag) to get a solution of 0.130 M H2SO4 (aq)? Write just the numerical answer with proper sig figs (no units) and do not put it in scientific notation. Make sure to record and submit the full work with units and sig figs in the separate file labeled 4 work.