Which of the following concerning the relative toughness of acids and also bases is/are correct? 1. As the acidity of the acid decreases, the basicity of the conjugate base boosts. 2. The hydronium ion is the strongest acid that have the right to be discovered in aqueous solution. 3. All acids classified as strong acids in aqueous solution have actually the very same acidity in a more acidic solvent choose acetic acid.
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Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in water?
The acid strength decreases in the series HBr>HSO4->CH3COOH>HCN>HCO3-. Which of the adhering to is the strongest base?
Which of the adhering to solutes, liquified in 1.0 kg of water, would certainly be expected to carry out the fewest pposts and to freeze at the highest temperature?
A solution has actually a pH of 10.20 at 25 degrees C. What is the hydroxide-ion concentration at 25 degrees C?
The pH of a solution of a strong base is 10.32 at 25 levels C. What is its hydronium-ion concentration?
Which of the adhering to statements is/are continual through the Bronsted-Lowry ideas of acids and bases?
In a(n) _____ soluition, at 25 levels C, the concentrations of H30 + and also OH- ions remajor equal as they are in pure water.
At 25 degrees C a solution has actually a hydroxide- ion concentration of 8.22 X 10^-5 M. What is its hydronium-ion concentration?
The acid toughness decreases in this series HBr> HSO4->CH3COOH>HCN>HCO3-. Which of the adhering to is the strongest base?
What is the hydroxide-ion concentration at equilibrium in a 0.66 M solution of ethylamine (C2H5NH2, Kb = 4.7 × 10-4) at 25oC?
The adhering to titration curve depicts the titration of a weak base via a solid acid. Which of the labeled points is the equivalence suggest.
A chemist prepares a buffer solution by mixing 70 mL of 0.15 M NH3 (Kb = 1.8 × 10-5 at 25 °C) and 50 mL of 0.15 M NH4Cl. Calculate the pH of the buffer.
A 0.20 M solution of a weak monoprotic acid is 0.22 % ionized. What is the acid-ionization consistent, Ka, for this acid?
What is the pH of an initially 0.428 M solution of a weak monoprotic acid that is 0.11 % ionized as soon as equilibrium is established? (assume Ca/Ka ≥102)
What is Kc for the following equilibrium? For phosphoric acid (H3PO4), Ka1 = 6.9 × 10-3, Ka2 = 6.2 × 10-8, and also Ka3 = 4.8 × 10-13.HPO42-(aq) + OH-(aq) PO43-(aq) + H2O(l)
What is the concentration of HCO3- in a 0.010 M solution of carbonic acid, H2CO3? For carbonic acid, Ka1 = 4.2 × 10-7 and also Ka2 = 4.8 × 10-11.
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What is the hydronium-ion concentration of a soultion developed by combining 400. ml of 0.21 M HNO3 via 600. ml of 0.10 M NaOH at 25 degrees C.