A solution is prepared by adding 20.0 mL of 0.15 M HCl to 80.0 mL of 0.20 M NH3. Ka(NH4+)= 5.8 x 10-10
a. Is this solution a buffer? Why or why not?
b. What is the pH of the solution?
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A solution is prepared by adding 20.0 mL of 0.15 M HCl to 80.0 mL of...
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(1 point) A buffer solution is prepared by adding 20.0 mL of 0.100 M sodium hydroxide solution to 50.0 mL of 0.100 M acetic acid solution. What is the pH of the buffer?
A 20.0-mL sample of 1.50 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 12.00 mL of acid have been added to ammonia? Kb for NH3 = 1.8 × 10–5 5.93 9.30 8.06 9.07 10.45
A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? Ka = 1.7
1. What is the pH of a buffer consisting of 0.30 M CH3COOH & 0.20 M NACH:COO? Ka= 1.8 x 10-5 2. What is the pH of the buffer with 0.10 M NH3 and 0.20 M NH4NO3? Kl = 1.8 x 10-5 3. What is the pH of a buffer formed from combining 10 mL of 0.250 M HCl with 90 mL of 0.150 M NH3? (K = 1.8 x 10-) 4. Calculate the pH of the solution that results...
A solution is prepared by mixing 20.0 mL of 0.050 M acetic acid and 10.0 mL of 0.100 M HCl. What is the pH of the solution? ( Ka acetic acid = 1.8 x 10-5) A. 2.36 B. 0.22 C. 1.48 D. 1.00 E. 0.48
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