8. 20.0 mL of 0.0155 M NaX is titrated with 0.0245 M HCl. The pH at the equivalence point is 4.25. a. Calculate Ka for HX. Answer: b. Calculate the pH after 35.34 mL HCl is added. Answer:

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A: Detail solution is given below

Q: 5) 6) O2(g) Al(s) + Ba(CIO3)2(aq) + ->> Al₂O3(s) Na3PO4(aq) Ba3(PO4)2(s) + NaClO3(aq)

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Q: e expression for Kc is

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A: Below attached file showing the details answer.  All the best.

Q: valence electron configuration

A:

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A: We can calculate equilibrium constant by using equation ∆G°= -R T lnK Where  ∆G°= Gibbs free energy…

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A: Given, □G° = -12.3 kJ/mol □G = -41.4 kJ/mol Relationship  □G = □G° + RT×ln(Q)

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Q: ! Given AG°f [NO] = 87 kJ/mol and AG°f [N20] = 104 kJ/mol, what is AG for the following reaction? 2…

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Q: Calculate AG in kJ-mol-1 at 298 K for the following reaction: 2 A(g) + B2(g) → 2 AB(s) AGO = -95…

A: Given-> ∆G°= -95 Kj/mole = -95000 J/mole (1KJ = 1000 J) P(A) = 0.155 atm P(B2) = 0.535 atm

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A: Below attached file showing the details answer.  All the best.

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :-  Ka for weak acid (HA) = 1.60 × 10-10  To determine :  Kb of its conjugate base (A-)

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.