Balance the following equations. (Use the smallest whole numbers possible. Enter 1 where appropriate - do not leave any answer box blank.) Ticla() + H20() - TiO2(s) HCI(ag) (b) B2S3(s) + H20() - | H3BO3(aq) +O HyS(g) (c) Fe(OH)3(s) + H2504(aq) - Fez(SO4)3(aq) + H20()

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Write chemical equations for the acid-base reactions that occur when solutions of the following substances are mixed: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) a H₂O and F + bOH and H₂PO4 CC6H5N (pyridine, a base) and HCHO2 (formic acid) + +

You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?

Much of the sulfur used in the United States comes from the hydrogen sulfide contaminant that makes "sour" natural gas smell bad. Hydrogen sulfide is separated from the other components of natural gas mostly by taking advantage of its acid-base reaction with aqueous ethanolamine: HO(CH,),NH,(aq)+H,S(g) → HO(CH,),NH,(aq)+HS (aq) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 167.6 mL of ethanolamine solution and 20.9 g of hydrogen sulfide gas each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature A B C D 5.0 L 5.0 L 5.0 L 5.0 L 49, °C 48. °C 51. °C 50. °C X initial rate of…

Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. Be sure to include the proper phases for all species within the reaction. CaBr2(aq)+AgNO3(aq) --->

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

What is the percent acetic acid in a 50.0 mL sample, which required 45.0 mL of a 0.1466 M NAOH to reach the equivalence point? (The sample solution has a density of 1.090 g/mL.) CH;CO,H(aq) - N2OH(aq) – NaCH;CO,(aq) - H,0(1)

balance equations and write net ionic equations of them. Thank you so much (a) Zn (s) + HCl(aq) -----> ZnCl2 (aq) + H2(g) (b) Na (s) + H2SO4 (aq) -----> Na2SO4 (aq) +H2(g) (c) AgNO3(aq)+ KCl(aq) ----> AgCl(s) + KNO3(aq) (d) NaHCO3 (aq) + HBr (aq) ----> NaBr (aq) + H2O (l) + CO2 (g)

8. LIOH (aq) CuCro, (aq) → +