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Which of the following barium salts should dissolve in a strong acid, such as HCL:
Ba(OH)2,
BaSO4, or
BaCO3
(Select all that apply.)
Step by step
Solved in 5 steps
- What volume, in milliliters, of 0.210 M NaOH should be added to a 0.125 L solution of 0.025 M glycine hydrochloride (p?a1=2.350, p?a2 = 9.778) to adjust the pH to 2.61? Please explain. Please type answer note write by hend.What is the pH at the equivalence point in the titration of a 18.3 mL sample of a 0.302 M aqueous nitrous acid solution with a 0.362 M aqueous barium hydroxide solution?pH = Submit AnswerAn aqueous solution contains 0.414 M ethylamine (C2H5NH2).How many mL of 0.214 M nitric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.500? Answer:_____
- An aqueous solution contains 0.399 M dimethylamine ((CH3)2NH).How many mL of 0.369 M hydrochloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.500? (answer is 110 mL)From their Kb values, which of the following bases would be best for preparing a buffer of pH 9.00: (i) NH3 (ammonia, Kb = 1.8 3 1025), (ii) C6H5NH2 (aniline, Kb = 4.0 3 10210), (iii) H2NNH2 (hydrazine, Kb = 9.5 3 1027), (iv) C5H5N (pyridine, Kb = 1.6 3 1029)?Which of the following aqueous solutions are buffer solutions? (Select all that apply.) 0.27 M HBr + 0.22 M KBr 0.13 M HF + 0.19 M NaF 0.38 M HClO + 0.27 M NaClO 0.33 M NH4Br + 0.39 M NH3 0.19 M Br(OH)2 + 0.22 M BaBr2
- Example 2What is the pH of the solution that results when 0.093 g of Mg(OH)2 Ksp = 7.1 × 10–12 is mixed with(a) 75.0 mL of 0.0500 M HCl?(b) 100.0 mL of 0.0500 M HCl?(c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?The OH– concentration in a solution of 0.0100 M NaClO is 5.9×10–5 M. What is the value of Kb for for ClO–?Need solution urgently 125mL of an alkaline water sample containing 128 ppm carbonate and 40ppm hydroxide in terms of CaCO_(3) equivalent its titrated against 0.20NHCl using methyl orange as the indicator.What will be the titre value (in ml unit)?
- (clear handwritten answer please) 29.0 mL sample of a 0.441 M aqueous hypochlorous acid solution is titrated with a 0.429 M aqueous barium hydroxide solution. What is the pH at the start of the titration, before any barium hydroxide has been added?A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notationHow many grams of solid barium acetate, Ba(C₂H₃O₂)₂ must be added to 500.0 ml of 0.390M acetic acid in order to form a buffer with a pH = 4.85?Answer: ___ grams of Ba(C₂H₃O₂)₂