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- According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?The balanced molecular equation for complete neutralization of H 2SO 4 by KOH in aqueous solution is H2SO4 (aq) + 2КОН (аq) — 2H20 (I) + К2S04 (s) B H2SO4 (aq) + 20H- (aq) → 2H2O (I) + SO42- (aq) (C) 2H+ (aq) + 20H- (aq) → 2H2O (I) D H2SO4 (aq) + 2KOH (aq) – 2H2O (I) + K2SO4 (aq) 2H+ (aq) + 2KOH (aq) → 2H2O (I) + 2K+ (aq) E.Reaction 4 BaCl,(aq): Na,SO,(aq): BaCl,(aq) + Na,SO,(aq) → Balance Equation: Observations: Type of Reaction: Reaction 5 FeCl,(aq): NaOH(aq): Balance equation: FeCl;(aq) + NaOH(aq) → Observations: Type of Reaction: Reaction 6 NaHCO,(aq): HCI(aq): Balance Equation: NAHCO,(aq) + HC1(aq) → Observations: Type of Reaction: Reaction 7 (1) Pb(NO3);(aq): (2) KI(aq): . Balance equation: Pb(NO,);(aq) + KI(aq) → Mass of test tube 1 and test tube 2 + beaker:_ Mass of the test tube that contains products + an empty test tube + a beaker: 58
- Adding acid to the buffer, NH3-NH4*, will produce this (net ionic) reaction: H*(aq) +OH(aq)=H₂O(1) H*(aq)+NH4*(aq) NH3(aq)+H₂(g) O H*(aq) + NH4+ (aq)=NH5²+ (aq) O H*(aq)+NH3(aq)=NH4+ (aq)Reaction 5 FeCl,(aq): NaOH(aq): Balance equation: FeCl,(aq) + NaOH(aq) - > Observations:Four different solutions were prepared at the same concentration: HCl(aq), HF(aq), NaOH(aq), and NH3(aq) When the pH values were measured, the solutions showed different pH values: (1) pH = 3.1 (2) pH = 5.8 (3) pH = 8.4 (4) pH = 12.8 Match each of the solutions with the measured pH values. Explain. solution pH value HCl(aq) ? HF(aq) ? NaOH(aq) ? NH3(aq) ?
- Reaction Acid-base neutralization reaction? 2 N2OH(aq) + Cacl,(aq) → 2 NaCI(aq) + Ca(OH),(aq) Reaction Acid-base neutralization reaction? H,SO,(aq) + 2 NaOH(aq) → 2 H,0(1) + Na,So,(aq)The solvation of calcium carbonate in water is shown. CaCO3 (s) + H₂0¹ (aq) = Ca²+ (aq) + HCO3 (aq) + H₂O(1) Keq = 71 Use this information to compare the grams per liter solubility of CaCO3 in pure water, a H₂O+ (aq) solution with a pH of 3.00, and a H3O+ (aq) solution with a pH of 1.00. The Ksp for CaCO3 is 3.36 × 10-⁹ solubility in pure water: 5.805 X10-3 solubility in a solution with a pH of 3.00: solubility in a solution with a pH of 1.00: g/L g/L g/LSodium 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 50.mL of a 0.027M 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.
- 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 man suffering from indigestion can be considered to be 50.mL of a 0.081 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.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 150.mL of a 0.053 M 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.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 CO2gas 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.