The solubility of 1-naphthylamin,
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General Chemistry: Principles and Modern Applications (11th Edition)
- Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forward50)arrow_forwardWrite the chemical reactions whose equilibrium constants are Kp and Ką for imidazole (C,H,N,) and imidazole hydrochloride (C,H,N,H*CI¯), respectively. K, reaction: 2.865 Incorrect K, reaction: 2.323 Incorrect Calculate the pH of a solution prepared by mixing 1.60 g of imidazole with 1.60 g of imidazole hydrochloride and diluting to 100.0 mL. The pKą of imidazole hydrochloride is 6.993. 2.07 pH Incorrect Calculate the pH of the solution if 2.00 mL of 1.06 M HCIO, are added. pH = Incorrect How many milliliters of 1.06 M HCI,, should be added to 1.60 g of imidazole to give a pH of 6.993? 2.865 volume: mL. Incorrectarrow_forward
- Benzoic acid is a weak acid that has antimicrobial properties. Its sodium salt, sodium benzoate, is a preservative found in foods, medications, and personal hygiene products. Benzoic acid ionizes in water: C6H5COOH(aq) ⇌ C6H5COO−(aq) + H+(aq) The pKa of this reaction is 4.2. In a 0.66 M solution of benzoic acid, what percentage of the molecules are ionized?arrow_forwardThe value of K, for acetylsalicylic acid (aspirin), HC,H,O4, is 3.00×10-4 Write the equation for the reaction that goes with this equilibrium constant. (Use H3O+ instead of H*.) + +arrow_forwardA patient presents itself to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 5.4×10-6 M and bicarbonate ion (HCO3-) 9.917 ×10-5 M Ka = 4.3 × 10-7 H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?arrow_forward
- 4arrow_forwardWhat are the molar concentrations of acetic acid (CH3COOH) and sodium acetate (CH3COONa) in an aqueous solution buffered at a pH of 4.22 that has a freezing point of −2.87 °C? Assume complete dissociation of sodium acetate and a density of 1.02 g/mL for the solution. The p?a for CH3COOH is 4.75.arrow_forwardThe concentration of acetylcholine (a neurotransmitter) in a sample can be determined from the pH changes that accompany its hydrolysis. When the sample is incubated with the enzyme acetylcholinesterase, acetylcholine is converted to choline and acetic acid, which dissociates to yield acetate and a hydrogen ion. CНз CHз Нао — сHz— CH "N— снз но-сн— сH,-"N-CH; + CH;— с-о+ н* CH3-C-0- сHз CHз Choline Acetylcholine Acetate In a typical analysis, 11 mL of an aqueous solution containing an unknown amount of acetylcholine had a pH of 7.70. When incubated with acetylcholinesterase, the pH of the solution decreased to 6.89. Assuming there was no buffer in the assay mixture, determine the number of moles of acetylcholine in the 11 mL sample.arrow_forward
- 5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5arrow_forwardThe acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 0.060 M . Express your answer using two significant figures. part B Calculate the equilibrium concentration of C6H5COO−C6H5COO− in the solution if the initial concentration of C6H5COOHC6H5COOH is 0.060 MM . Express your answer using two significant figures.arrow_forwardAmino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?arrow_forward
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