10:59How to Determine if Salt is Acidic, Basic, or Neutral Example, Problem, Shortcut, Explained QuestionConquer Chemistry847views
13:33Acid–base properties of salts | Acids and bases | AP Chemistry | Khan AcademyKhan Academy506views
14:15pH of salt solutions | Acids and bases | Chemistry | Khan AcademyKhan Academy Organic Chemistry441views
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a) LiC2H3O2 b) C6H5NH3Br817views2comments
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a) Co(HSO4)2 b) Sr(HSO3)2577views3comments
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a. C3H7NH3F637views2rank5comments
Multiple ChoiceDetermine the pH of a 0.55 M NaCN solution. The Ka of hydrocyanic acid, HCN, is 4.9 x 10-10.1730views1rank11comments
Multiple ChoiceWhich of the following compounds would decrease the pH of solution?a) SrBr2 b) KSH c) NaN3 d) NiP e) Hg2Cl2214views2rank
Multiple ChoiceWhich of the following compounds would increase the pH of solution?a) SrBr2 b) K c) NaN3 d) NiBr2 e) Hg2Cl2193views1rank
Multiple ChoiceWhich of the following compounds would have an increase in solubility when placed into an acidic solution? a) CaBr2 b) NaI c) KCN d) LiNO3 e) Hg2Br2200views1rank
Textbook QuestionA formic acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addition? Explain your answer. a. HCl b. NaBr c. NaCHO2 d. KCl2790views1rank
Textbook Question(b) If a limestone sculp- ture were treated to form a surface layer of calcium sul- fate, would this help to slow down the effects of acid rain? Explain.333views
Textbook QuestionLabel each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (c) NaClO4378views
Textbook QuestionLabel each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (b) acetonitrile, CH3CN582views
Textbook QuestionThe following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (c) Which M1H2O26n + ion 1n = 1,2, or 32 is the strongest acid, and which has the strongest conjugate base?256views
Textbook QuestionWould you expect zirconium(II) oxide, ZrO, to react more readily with HCl(aq) or NaOH(aq)?276views
Textbook QuestionArrange the following oxides in order of increasing acidity: K2O, BaO, ZnO, H2O, CO2, SO2.702views
Textbook QuestionChlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?538views1rank
Textbook QuestionAn element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (b) Do you think that element X is a metal, nonmetal, or metalloid?319views
Textbook QuestionAn element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (a) XCl4 reacts with water to form XO2 and another product. What is the likely identity of the other product?710views
Textbook QuestionWrite balanced equations for the following reactions: (a) boron trichloride with water351views
Textbook QuestionWrite balanced equations for the following reactions: (c) phosphorus pentoxide with water257views
Textbook QuestionWrite balanced equations for the following reactions: (d) arsenic trioxide with aqueous potassium hydroxide.343views
Textbook QuestionPyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (a) Write out the reaction that leads to this acidic pH.829views1rank
Textbook QuestionPredict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (c) Na2CO31037views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (e) Na2SO3.400views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (c) NaClO490views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (b) NaBr842views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AlCl3381views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (d) 3CH3NH34NO3381views
Textbook QuestionAn unknown salt is either NaF, NaCl, or NaOCl. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08. What is the identity of the salt?851views
Textbook QuestionAn unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 0.100 M solution of the salt is neutral, what is the identity of the salt?628views
Textbook QuestionDetermine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3-1234views
Textbook QuestionIndicate whether each of the following statements is correct or incorrect. (d) K+ ion is acidic in water because it causes hydrating water molecules to become more acidic.323views
Textbook QuestionDetermine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+666views
Textbook QuestionDetermine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+377views
Textbook QuestionDetermine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+542views
Textbook QuestionDetermine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+653views
Textbook QuestionDetermine if each compound is more soluble in acidic solution than it is in pure water. Explain. c. AgCl3375views
Textbook QuestionDetermine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li+1232views
Textbook QuestionDetermine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO21951views
Textbook QuestionDetermine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3601views
Textbook QuestionArrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH3169views
Textbook QuestionWhich of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) AgBr456views
Textbook QuestionWhich of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (b) Fe(OH)3632views
Textbook QuestionWrite a balanced net ionic equation for the principal reaction in solutions of each of the following salts. In each case, identify the Brønsted–Lowry acids and bases and the conjugate acid–base pairs. (a) Na2CO3523views
Textbook QuestionClassify each of the following ions according to whether they react with water to give a neutral, acidic, or basic solution. (a) F-508views
Textbook QuestionClassify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for values of equilibrium constants. (a) Fe1NO323711views
Textbook QuestionCalculate Ka for the cation and Kb for the anion in an aqueous NH4CN solution. Is the solution acidic, basic, or neutral?704views
Textbook QuestionThe hydrated cation M1H2O26 3 + has Ka = 10-4, and the acid HA has Ka = 10-5. Identify the principal reaction in an aqueous solution of each of the following salts, and classify each solution as acidic, basic, or neutral. (a) NaA346views