Does the pH increase, decrease, or remain the same when NH4Br is added to an aqueous solution of NH3? Explain clearly your reasoning using appropriate equilibrium(s) and equation(s).

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species NO2 |(Choose one) HNO, 2 H,O 4 103 5 НСООН (Choose one) ▼ OH (Choose one) HIO3 (Choose one) НСОО 7

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species so 103 OH F 2- HSO4 HIO3 H₂O HF relative pH of 0.1 M aqueous solution 6 (Choose one) ▼ 8 (highest) 7 (Choose one) 1 (lowest) (Choose one) ▼ (Choose one) X ? 圖 ola

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An analytical chemist is titrating 221.9 mL of a 0.9800M Solution of propionic acid (HC,H,CO,) with a 0.8400OM solution of NaOH. The pK, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 190.2 mL of the NAOH SOlution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH Solution added. Round your answer to 2 decimal places. pH = ?

Kal Ascorbic acid (H₂CH₂O) is a diprotic acid. The acid dissocation constants for H₂CH₂O are K₁1 = 8.00 × 10-5 and K₁2 = 1.60 x 10-12. Determine the pH of a 0.136 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. H₂C₂H₂O] = [HC₂H₂OT] = [C₂H₂O²] = M M M

Calculate the pH and degree of hydrolysis in the 0.02 M solution of sodium acetate

The equilibrium constant expression for the second ionization step of phosphoric acid (Ka2) will contain __________ in the numerator (top). Adding heat to an endothermic reaction will _________.     decrease the amount of product     increase the amount of reactants     shift the equilibrium to the left     all of the above     none of the above

.030 moles of a weak acid, HA, was dissolved in 2.0L of water to form a solution. At equilibrium the concentration of HA was found to be .013 M. Determine the value of Ka for the weak acid.

Consider an unknown solution. Experimental work determined that the aqueous solution contained some intact molecule as well as product ions. When exposed to red cabbage juice the solution turned pink. Choose all molecules that align with the experimental results. NaOH O Ca(OH)2 O NH3 HC2H3O2 H3PO4 HCI O HNO3