(a)
Interpretation:
It should be determined whether the carbonate transposition will be effective for detecting SO42- from BaSO4 or not.
Concept introduction:
Carbonate transposition is a reaction which leads to determine that the slightly soluble solids’ aqueous medium anion concentration is sufficient for qualitative analysis.
(b)
Interpretation:
It should be determined whether carbonate transposition will be effective for detecting Cl- from AgCl or not.
Concept introduction:
Carbonate transposition is a reaction which leads to determine that the slightly soluble solids’ aqueous medium anion concentration is sufficient for qualitative analysis.
(c)
Interpretation:
It should be determined whether the carbonate transposition will be effective for detecting F- from MgF2 or not.
Concept introduction:
Carbonate transposition is a reaction which leads to determine that the slightly soluble solids’ aqueous medium anion concentration is sufficient for qualitative analysis.
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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- Your answer is partially correct. Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = i 9.08 eTextbook and Media Save for Later Attempts: 1 of 3 used Submit Answerarrow_forward57. The pH of normal, unpolluted rainwater is controlled by carbonic acid equilibrium: COz(g) > COz(aq) + H2CO3° (a) Write down the equilibrium expressions (K) for the three carbonate reactions. Mat 16 (b) What is the pH of rainwater in equilibrium with atmospheric CO2 (Pco2 = 10-3.5 atm)? Assume that the pH will be controlled by dissociation of carbonic acid (H₂CO3º) to HCO3- (i.e., [HCO3] [H*]). Hence need consider only the first and the second reactions in the series of carbonate reactions. Known Kco2 = 10-1.46, K₁ = 10-6.35, pH = -log[H*]. (INATE) 14arrow_forwardSome kidney stones form by the precipitation of calciumoxalate monohydrate (CaC₂O₄H₂O, Kₛₚ=2.3X10⁻⁹). The pH of urine varies from 5.5 to 7.0, and the average [Ca²⁺] in urine is 2.6X10⁻³ M.(a) If the [oxalic acid] in urine is 3.0X10⁻¹³ M, will kidneystones form at pH =5.5?(b) At pH= 7.0?(c) Vegetarians have a urine pH above 7. Are they more or lesslikely to form kidney stones?arrow_forward
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