Understanding connections between descriptions of wea... When a 0.033M aqueous solution of a certain acid is prepared, the acid is 4.0% dissociated. Calculate the pH of the solution. Round your answer to 2 decimal places. pH = [| dlo
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- A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.Due to the pandemic Covid-19, the uses of hand sanitizers are very important among us. Predict and explain the colour of the solution and pH value when red cabbage indicator was added to the hand sanitizers.The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively equal to
- A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the KB of NH3 is 1.86 × 10^⁻5, determine the pH of the resultant solution. (You may assume the volume is unchanged.)A solution is prepared at 25\deg C that is initially 0.22M in nitrous acid HNO2, a weak acid with = Ka\times 4.510-4, and 0.049M in potassium nitrite KNO2. Calculate the pH of the solution.TRIS (also known during medical use as THAM) is an organic compound used extensively in biochemistryand molecular biology as a component of buffer solutions, especially for solutions of nucleic acids. At 37oC,-7body temperature, its Kb value is 5.13 x 10 . What is the approximate ratio of acid to base at pH 7.4, the pH ofblood?
- Sodium acetate, CH3COONa was hydrolysed in water, H2O. Show thereaction equations involved. What is the effect of the salt on the pH of thissolution?A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) What would the pH of the solution be if 0.020 mol HCl added to the solution in a? What would the pH of the solution be if 0.15 mol HCl added to the solution in a? What would the pH of the solution be if 0.17 mol HCl added to the solution in a?.A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) a) What is the pH of such solution?b) What would the pH of the solution be if 0.020 mol NaOH added?c) What would the pH of the solution be if 0.15 mol NaOH added to the solution in a?d) What would the pH of the solution be if 0.17 mol NaOH added to the solution in a? e) What would the pH of the solution be if 0.020 mol HCl added to the solution in a? f) What would the pH of the solution be if 0.15 mol HCl added to the solution in a?g) What would the pH of the solution be if 0.17 mol HCl added to the solution in a?
- A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) a) What is the pH of such solution?. Single line text.Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) 1) What is the pH of such solution? 2)What would the pH of the solution be if 0.17 mol NaOH added to the solution in 1? 3)What would the pH of the solution be if 0.020 mol HCl added to the solution in 1? 4)What would the pH of the solution be if 0.15 mol HCl added to the solution in 1? 5)What would the pH of the solution be if 0.17 mol HCl added to the solution in 1?