10:59How to Determine if Salt is Acidic, Basic, or Neutral Example, Problem, Shortcut, Explained QuestionConquer Chemistry841views
13:33Acid–base properties of salts | Acids and bases | AP Chemistry | Khan AcademyKhan Academy500views
14:15pH of salt solutions | Acids and bases | Chemistry | Khan AcademyKhan Academy Organic Chemistry432views
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a) LiC2H3O2 b) C6H5NH3Br815views2comments
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a) Co(HSO4)2 b) Sr(HSO3)2574views3comments
Multiple ChoiceDetermine if each of the following compounds will create an acidic, basic or neutral solution.a. C3H7NH3F636views2rank5comments
Multiple ChoiceDetermine the pH of a 0.55 M NaCN solution. The Ka of hydrocyanic acid, HCN, is 4.9 x 10-10.1720views1rank11comments
Multiple ChoiceWhich of the following compounds would decrease the pH of solution?a) SrBr2 b) KSH c) NaN3 d) NiP e) Hg2Cl2210views2rank
Multiple ChoiceWhich of the following compounds would increase the pH of solution?a) SrBr2 b) K c) NaN3 d) NiBr2 e) Hg2Cl2191views1rank
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) Hg2Br2198views1rank
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. KCl2776views1rank
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.329views
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) NaClO4374views
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, CH3CN577views
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?253views
Textbook QuestionWould you expect zirconium(II) oxide, ZrO, to react more readily with HCl(aq) or NaOH(aq)?273views
Textbook QuestionArrange the following oxides in order of increasing acidity: K2O, BaO, ZnO, H2O, CO2, SO2.696views
Textbook QuestionChlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?525views1rank
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?314views
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?694views
Textbook QuestionWrite balanced equations for the following reactions: (a) boron trichloride with water347views
Textbook QuestionWrite balanced equations for the following reactions: (c) phosphorus pentoxide with water255views
Textbook QuestionWrite balanced equations for the following reactions: (d) arsenic trioxide with aqueous potassium hydroxide.339views
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.819views1rank
Textbook QuestionPredict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (c) Na2CO31029views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (e) Na2SO3.396views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (c) NaClO486views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (b) NaBr835views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AlCl3379views
Textbook QuestionPredict whether aqueous solutions of the following substances are acidic, basic, or neutral: (d) 3CH3NH34NO3378views
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?849views
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?618views
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. NO3-1224views
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.320views
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+660views
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+374views
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+538views
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+648views
Textbook QuestionDetermine if each compound is more soluble in acidic solution than it is in pure water. Explain. c. AgCl3367views
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+1228views
Textbook QuestionDetermine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO21939views
Textbook QuestionDetermine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3596views
Textbook QuestionArrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH3159views
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) AgBr452views
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)3628views
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) Na2CO3514views
Textbook QuestionClassify each of the following ions according to whether they react with water to give a neutral, acidic, or basic solution. (a) F-503views
Textbook QuestionClassify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for values of equilibrium constants. (a) Fe1NO323706views
Textbook QuestionCalculate Ka for the cation and Kb for the anion in an aqueous NH4CN solution. Is the solution acidic, basic, or neutral?699views
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) NaA342views