1. Which equation depicts hydrogen phosphate ion behaving as a Bronsted-Lowry ba
ID: 635733 • Letter: 1
Question
1. Which equation depicts hydrogen phosphate ion behaving as a Bronsted-Lowry base in water? a. HPO (a) +H20() PO (aq)+H:O (aq) b. HP042 (aq) + OH (aq)-PO-(aq) + H2O(1) ? HP042-(aq) + H20(1)?12PO'(aq) + OH(aq) 2 HP042 (aq) + 02-(aq) PO,'-(aq) + H20(1) e. 2 HPO (aq)+ HO)2 HO)+ P:O+(s) 2. What is the phH of 0.50 M HOCIa)? ( of HOCI-3,5 x 10) a.3.88 b. 6.54 c. 7.46 7.74 e. 10.12 3. Which of the following combinations would be best to buffer an aqueous solution at a pH of 2.02 aHPO and H POs, Kal -7.5x 10- b. HNO2 and NO2, K -4.5x 104 c. CHCO H and CH COO, K 1.8 x 10- d. HPO4 and HPO2K 6.2x 10 e. NH and NHs, K5.7x10-10 4. A buffer is composed of 0.400 mol H:PO, and 0.400 mol HPO,2 diluted with water to a volume of 1.00 L. The pH of the buffer is 7.210. How many moles of HCI must be added to decrease the pH to 6.710? a. 3.60 mol b. 0.400 mol c. 0.360 mol 0.327 mo 0.208 molExplanation / Answer
The correct answer is option (a)
pH= -1/2( logC + logKa )
pH= -1/2( log0.50 + log3.5 x 10-8)
pH= -1/2(-0.301 - 7.456)
pH= 3.88
Hope it helped..Good luck??
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