Phosphoric acid, H3PO4, is a polyprotic acid. What is the THIRD ionization reaction for phosphoric acid in water? HPO (aq) → H+ (aq) + PO³ (aq) ○ H3PO4 (aq) → 3 H+ (aq) + PO¾- (aq) 4 H₂PO (aq) → HPO²¼¯ (aq) + H+ (aq) H3PO4 (aq) → H₂PO (aq) + H+ (aq)
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- The pH of an aqueous solution of 0.1690 M hydrosulfuric acid, H₂S (aq), isThe pH of an aqueous solution of 0.176 M tellurous acid, H2TeO3 (aq), isAssume you titrated to the endpoint 0.10 moles of HA (weak, monoprotic acid) with a solution of sodium hydroxide, NaOH(aq), of unknown concentration. The initial volume of NaOH(aq) in the buret was 5.00 mL, and the final volume of NaOH(aq) in the buret was 45.00 mL. What is the concentration, in molarity, of the NaOH solution used?
- The pH of an aqueous solution of 0.137 M sodium hypochlorite, NaClO (aq), is ________________ This solution is: ________ (ACIDIC, BASIC, OR NEUTRAL?)If weak acids ionize only a few percent in aqueous solution, why is it possible to fully neutralize a weak acid by reacting it with the stoichiometric equivalent of sodium hydroxide solution, NaOH(aq)?To measure the amount of calcium carbonate CaCO3 in a seashell, an analytical chemist crushes a 4.500g sample of the shell to a fine powder and titrates it to the endpoint with 172.mL of 0.380M hydrogen chloride HCl solution. The balanced chemical equation for the reaction is: →+2HClaq CO2−3aq + H2CO3aq 2Cl−aq What kind of reaction is this? Percipitation, acid-base, or redox Calculate the mass percent of CaCO3 in the sample. Be sure your answer has the correct number of significant digits.
- When acidulated water (dil.H2SO2solution) is electrolysed, will the pH of the solution be affected? Justify your answer.Phosphoric acid, H3PO4 (aq), is found in soda. Write the balanced chemical equation for the neutralization of phosphoric acid with NaOH.Complete and balance each of the following equations for acid-base reactions. H2SO4(aq)+Ca(OH)2(aq)→H2SO4(aq)+Ca(OH)2(aq)→ Express your answer as a chemical equation. Identify all of the phases in your answer.
- Assuming the base completely dissociates in water, what is the pH of a 5.70 g/L solution of Ba(OH) 2 (aq) ?Balanced equation for: AgNO3(aq) + NaOH(aq)A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.