Cyclohexanecarboxylic acid, C6H11COOH (pKa 4.90), is only slightly soluble in water, but its sodium salt,C6H11COO-Na+, is quite soluble in water. Describe the solubility of cyclohexanecarboxylic acid in solutions of sodium hydroxide, sodium bicarbonate (NaHCO3), and sodium carbonate (Na2CO3). The pKa values for the conjugate acids of sodium hydroxide, sodium bicarbonate (NaHCO3), and sodium carbonate (Na2CO3) are 15.7, 6.36, and 10.33, respectively. Aqueous NaOH: _________soluble, insoluble, or slightly soluble Aqueous NaHCO3: _________soluble, insoluble, or slightly soluble Aqueous Na2CO3: _________soluble, insoluble, or slightly soluble

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sangriamouse849Lv1

29 Sep 2019

Cyclohexanecarboxylic acid, C₆H₁₁COOH (pKa 4.90), is only slightly soluble in water, but its sodium salt,C₆H₁₁COO^-Na⁺, is quite soluble in water. Describe the solubility of cyclohexanecarboxylic acid in solutions of sodium hydroxide, sodium bicarbonate (NaHCO₃), and sodium carbonate (Na₂CO₃). The pKa values for the conjugate acids of sodium hydroxide, sodium bicarbonate (NaHCO₃), and sodium carbonate (Na₂CO₃) are 15.7, 6.36, and 10.33, respectively.

Aqueous NaOH: _____soluble, insoluble, or slightly soluble

Aqueous NaHCO₃: _soluble, insoluble, or slightly soluble

Aqueous Na₂CO₃: _____soluble, insoluble, or slightly soluble

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To separate a mixture of benzoic acid and fluorene, we are going to use an acid-base extraction technique. Most carboxylic acids are insoluble or slightly soluble in water, but they are highly soluble in dilute aqueous sodium hydroxide because the organic acid reacts with the base and produces carboxylate ions, a polar species. In a mixture of a carboxylic acid and an organic compound, the acid may be selectively removed from an organic solvent by extracting with a dilute NaOH solution. After separating the organic and aqueous layers, the carboxylic acid may be recovered from the aqueous solution by adding HCl, which causes precipitation of the carboxylic acid. Draw two structures below.To separate a mixture of benzoic acid and fluorene

Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43Ã10â7 and Ka2=4.73Ã10â11. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation

NaHCO3(aq)+HCl(aq)âH2CO3(aq)+NaCl(aq)

Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate solutions are methyl orange and phenolphthalein.

Part A

What volume of 0.130 M HCl is required for the complete neutralization of 2.00 g of NaHCO3(sodium bicarbonate)?

What volume of 0.170 M HCl is required for the complete neutralization of 1.50 g of Na2CO3(sodium carbonate)?

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.190 g of this sample requires 23.98 mL of 0.100 MHCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?