f) pH of 0.35 M CH3CH2NH2
g) pH of 0.35 M NaHSO4
h) pHos 0.35 M CH3CH2NH3Br
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Calculate pH of 0.35 M CH3CH2NH2 0.35 M NaHSO4 0.35 M CH3CH2NH3Br
2) Calculate the pH of each of the following solutions. a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
calculate the ph of the following solutions there is 3 different problems so make sure to click on the picture! thank you f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3B
Please write out equation used and indicate the values used where in each equation. ICE tables, where applicable. 2) Calculate the pH of each of the following solutions. (5 pts each) a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
2. Calculate the pH at the equivalence point when 30 mL of 0.206 M CH3CH2NH2, is titrated with 0.559 M HBr.
What is the pH of a 1.00 M solution of sodium sulfate (NaHSO4)? You can use the equilibrium constants from number 1 to figure out the answer. (Ka1 = large Ka2 = 1.2 x 10-2 ) -1.47 1.01 0.033 0.96 -0.96
Calculate the hydronium ion concentration and the pH when 15.0 mL of 0.35 M NH, is mixed with 15.0 ml. of 0.35 M HCI (K Concentration - 5.6 x 10 pH- kat 125°C, what is the total pressure in the back at equilibrium? What are the stures of the Lewis acid, the If you place of the complex in a 69.5 ml. Lewis base, and the complex? P(BF,) - Am P(CI 10) an P[(CH), O--BF,)- P(total) - atm
For 300.0 mL of a buffer solution that is 0.325 M in CH3CH2NH2 and 0.300 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
For 550.0 mL of a buffer solution that is 0.150 M in CH3CH2NH2 and 0.140 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of HCl.
For 250.0 mL of a buffer solution that is 0.295 M in CH3CH2NH2 and 0.275 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.