Voltmeter Wire +1.56 V NO3 K+ Zn Ag 1 M Zn(NO3)2 1 M AgNO3 2 Ag+ (aq) + Zn(8) 2 Ag(8) + Zn+ (aq) Under standard conditions, the galvanic cell shown above has a cell potential of +1.56 V using the reaction given. The salt bridge contains KNO3, which allows K+ ions and NO3 ions to move in the directions indicated. If KNO3 in the salt bridge is replaced with KOH, some Zn(OH)2 (8) precipitates in the Zn-Zn(NO3), half-cell. Which of the following best explains how the cell potential is affected as Zn(OH)2 (3) starts to precipitate, and why? A The cell potential increases because the concentration of Zn2+ (aq) decreases and Q, becomes smaller Ag+ B The cell potential decreases because the concentration of Zn2+ (aq) decreases and Q, becomes smaller. Agt? The cell potential increases because K+ ions replace Zn2+ ions and the reduction of K+ is more thermodynamically favored than the reduction of Zn2+. D The cell potential stays the same because Zn(OH), (3) is not part of the redox reaction responsible for the operation of the galvanic cell