Given the following data, Base K, NH3 1.8 x 10-5 CH3NH2 5.0 x 10 C6 H6 NH2 4.2 × 10-10 Calculate the pH of 0.68 M solutions of 1. NH4NO3 pH = 2. CH3NH3 NO3 pH = 3. СеHsNH3NОз pH =

Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. CH;C00 HCN (aq) CHĄCOOH CN Brønsted-Lowry | Brønsted-Lowry Brønsted-Lowry | Bronsted-Lowry { In this reaction: The formula for the conjugate )of CH3COO¯ is The formula for the conjugate| of HCN is

[H3O+1] = 10-PH [OH-1] = 10-pOH [H3O+1][OH1] = 10-14 pH - log [H3O+1] = %3D pOH = - log [OH-] pH + pOH = 14 %3D %3D What will be the pH if 0.00150 moles of HCl is added to 1.00L of water ? The reaction gives the conversion factor HCI + H2O H3O+1 + CI1 start: 0.00150 equil: O A. 1.5000 В. 2.5223 C. 2.824 D. 3.125 Е. 6.502

N2H4 is a weak base. approximately how many moles of N2H4 are required for each mole of N2H5+ to create a solution with a pH equal to 8.5?

Consider 0.100 M aqueous solutions of the following chemicals. Rank them in increasing order of pH (lowest pH to highest pH). HCIO₂ Rationale Ranking: NaF CH3CH₂NH3CI KCH3COO NH3

1 M NaOH has the same pH as 1 M NH4OH. O True O False

The ?a of propanoic acid (C2H5COOH) is 1.34×10−5. Calculate the pH of the solution and the concentrations of C2H5COOHand C2H5COO− in a 0.515 M propanoic acid solution at equilibrium.

Determine the [OH-], pH, and pOH of a solution with a [H+] of 4.7 × 10-¹² M at 25 °C. [OH-] = pH: = POH Determine the [H+], pH, and pOH of a solution with an [OH-] of 6.7 x 10-7 M at 25 °C. [H+] = pH : = = POH = M M

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Which of these acids has the lowest pH at equilibrium? Acid Ka HIO3 1.7 x10-1 HCIO2 1.1 x10-2 HCOOH 1.8 x10-4 CH3COOH 1.8 x10-5