Given that at 25.0 °C ● calculate ● -10 Ka for HCN is 4.9 × 10- and Kb for NH3 is 1.8 × 10-5, ● Kb for CN and K₂ for NH4+. Enter the K₁ value for CN- followed by the Ka value for NH4 separated by a comm + "

The beakers below depict the aqueous dissociations of weakacids HA (blue and green) and HB (blue and yellow); solvent molecules are omitted for clarity. If the HA solution is 0.50 L,and the HB solution is 0.25 L, and each particle represents 0.010mol, find the Kₐ of each acid. Which acid, if either, is stronger?

Please don't provide handwritten solution.....   Determine the pH for 0.35M solution of sodium formate, NaCHOO acid, HCOOH. ● Ka for formic acid, HCOOH is 1.80x10-4.

Given the following: H2S -> H + HS (K = 9.5x10^-8) and HS->H+S (K = 1.0x10^-19) Find the equilibrium constant for the following reaction: H2S-> 2H + S

γ -hydroxybutyric acid is a weak acid which is a naturally occurring neurotransmitter. Its calcium salt is used for narcolepsy treatment. A saturated solution of this salt, which we can represent as Ca(GHB)2 has a [Ca2+]=8.6×10−2molL−1 and a pH=8.98 . Assuming the salt is completely dissociated, calculate the Ka of γ -hydroxybutyric acid. please answer fast i give you upvote.

Given that at 25.0 °C K, for HCN is 4.9 × 10–10 K, for NH3 is 1.8 × 10-5, and calculate Ki, for CN and K, for NH4*. Enter the K1, value for CN followed by the K, value for H4*, separated by a comma, using two significant figures.

4. The equations and constants for the dissociation of three different acids are given below. HCO3 = H+ + CO?- K. = 4.2 x 10–7 -8 H;PO, = H+ + HPO- K. = 6.2 x 10 HSO, = H+ + SO?- Ka = 1.3 x 10–2 a. From the systems above, identify the conjugate pari that is best for preparing a buffer with a pH. of7.2. Explain your choice. b. Explain briefly how you would prepare the buffer solution described in (a) with the conjugate pair you have chosen. c. If the concentrations of both the acid and the conjugate base you have chosen were doubled, how would the pH be affected? Explain how the capacity of the buffer is affected by this change in concentrations of acid and base.

Nicole separately prepared solutions of FeSO4 and FeBr3 with concentrations 7.71×10-1 M and 3.77×10-2 M respectively. Calculate the p-value for all ions and substances in these solutions.

Calculate the pOH of a solution that results from mixing 32.09 mL of 0.18 M HCN(aq) with 33.8 mL of 0.19 M NaCN. The Ka value for HCN is 4.9 x 10-10.

16) Calculate the Ka (aq., 25 oC) of a 0.525 M weak monoprotic acid that is 6.45% ionized. a) 2.65 x 10–4​​b) 1.25 x 10–5​​c) 8.65 x 10–6​​d) 5.42 x 10–3​ ​​e) 2.33 x 10–3​​​​f) 7.22 x 10–4