# The ph of a 0.30 m solution of a weak acid is 2.67. what is the ka for this acid [Solved] Ka 1.510 Possibility E. Not one of the above Clarification: We suggest the response of equlibrium Weak ac.H HO Weak ac HO Initially weve 0.30 moles of acid in 1 L In equilibrium wed have: Weak ac.H HO Weak ac HO 0.30 x x x We now have the pH, the place we will obtanined the x, the [HO] within the equilibrium. pH = log [HO] [HO] = 10^(pH) [HO] = 10 = 2.1410 So lets decide the focus of the acid, within the equilibrium 0.30 2.1410 = 0.29786 [Weak ac.H] 2.1410 [HO] = Conjugate base (Weak ac.) Lets make the expression for Ka Ka = [Weak ac.] . [HO] / [Weak ac.H] Ka = x / 0.30 x Ka = (2.1410) / 0.29786 1.510

Clarification: Since its a weak acid its needed to write down the stability. The place the unknown acid will probably be HA. . Then with the equilibrium we will write the ICE desk (determine 1). The place we get hold of the equation: Now, weve to seek out X. To do that we will use the pH equation and the pH worth: Then weve to plug the values within the Ka equation:

Clarification: Since its a weak acid its needed to write down the stability. The place the unknown acid will probably be HA. . Then with the equilibrium we will write the ICE desk (determine 1). The place we get hold of the equation: Now, weve to seek out X. To do that we will use the pH equation and the pH worth: Then weve to plug the values within the Ka equation:

Ka 1.510 Possibility E. Not one of the above Clarification: We suggest the response of equlibrium Weak ac.H HO Weak ac HO Initially weve 0.30 moles of acid in 1 L In equilibrium wed have: Weak ac.H HO Weak ac HO 0.30 x x x We now have the pH, the place we will obtanined the x, the [HO] within the equilibrium. pH = log [HO] [HO] = 10^(pH) [HO] = 10 = 2.1410 So lets decide the focus of the acid, within the equilibrium 0.30 2.1410 = 0.29786 [Weak ac.H] 2.1410 [HO] = Conjugate base (Weak ac.) Lets make the expression for Ka Ka = [Weak ac.] . [HO] / [Weak ac.H] Ka = x / 0.30 x Ka = (2.1410) / 0.29786 1.510

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