The values of K a for hydrozoic acid ( HN 3) and hypobromous acid (HBrO) are given below. HN3 Ka = 1.9 x 10°s HBRO Ka = 2.0 x 10-9 If we mix 0.50 mol HN 3 and 0.50 mol NaBrO into a 1-L aqueous solution, which of the following statements is correct concerning the final solution at equilibrium after mixing? O a. The pH of the final solution is greater than 7 because K, (HN3) < K½( BrO" ). O b. The pH of the final solution is greater than 7 because K, (HN3) > K½(BrO"). O. The pH of the final solution is equal to 7 because the neutralization reaction between HN3 and NaBrO. O d. The pH of the final solution is less than 7 because K. (HN2) > KL( BrO" ).

A solution of three different weak acids is prepared and initially contains the following: |0.15 М HCIO Ka = 1.1 x 10-2 %3D 0.20 M HC,H5O2 Ka = 1.8 x 10-6 %3D |0.25 М НСgHsО |Ка3 1.0 х 10-10 What is the pH of the solution at equilibrium?

10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). If the resulting equilibrium pH was 1.4, what was the concentration of the HCl solution?

A patient presents to the emergency department in a very critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 4.0×10-4 M and bicarbonate ion (HCO3-) 3.062×10-3 M. Ka = 4.3 × 10-7 H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. a. Calculate the pH of the patients’ blood. b. Based on your answer would you say the patient suffered from Acidosis or Alkalosis

Select the mixture that is capable of tolerating the addition of a strong acid without altering the pH   Group of answer choices 1.0 M NH3 and 1.0 M NaCl 1.0 M HCl and 1.0 M NaCl 1.0 M HNO2 and 1.0 M NaNO2 1.0 M HF and 1.0 M NaCl

A certain weak base has a Kp of 8.60 x 10-7. what concentration of this base will produce a pH of 10.37? concentration: M

25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka of acetic acid is 1.8x10-5. What is the pH of the solution after adding NaOH?

HCIO is a weak acid (Ka = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.039 M in NaCIO at 25 °C? pH =

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Fill in the blanks to show how you would solve for the pH of a 0.10 M aqueous solution of the weak acid HA. For the table and the equilibrium expression, do not ignore x. 0.10 POH Initial Concentration (M) Change 0.10 - X Equilibrium 2x² K₂ = 0.10 - 2x 4x² HA(aq) X (0.10 - x)² + 2x (0.10-2x)² H₂O(l) + +