A buffer solution is made that is 0.386 M in HNO2 and 0.386 M in KNO2. If Ka for HNO2 is 4.50 × 10-4, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.110 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) Submit Answer Retry Entire Group 9 more group attempts remaining

A buffer solution is made that is 0.474 M in H₂CO3 and 0.474 M in KHCO3. If Kal for H₂CO3 is 4.20 × 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.119 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H†)

A buffer solution is made that is 0.339 M in HF and 0.339 M in KF. If K, for HF is 7.20 × 10-4, what is the pH of the buffer solution? pH =| Write the net ionic equation for the reaction that occurs when 0.088 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +

Chemistry (Part -3) =============

We have 500.0 mL of a buffer solution that is 0.697 M in NH3 and 0.380 M in NH4Cl. We add 500.0 mL of a solution 0.202 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?

A buffer solution is 0.416 M in H2 S and 0.245 M in NaHS. If K21 for H2S is 1.0 x 10-7, what is the pH of this buffer solution? pH =| A buffer solution is 0.376 M in N.HSO3 and 0.390 M in Na,SOg. If K, for HSO3 is 6.4 × 10-8, what is the pH of this buffer solution? pH =

A buffer solution is made that is 0.368 M in HCN and 0.368 M in KCN. If Ka for HCN is 4.00 × 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +

A buffer solution is made that is 0.485 M in HClO and 0.485 M in KClO. If Ka for HClO is 3.50x10^-8, what is the pH of the buffer solution? pH =  Write the net ionic equation for the reaction that occurs when 0.129 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)

A buffer solution is made that is 0.452 M in HC10 and 0.452 M in KC10. If K, for HC10 is 3.50 x 10-8, what is the pH of the buffer solution? pH : Write the net ionic equation for the reaction that occurs when 0.100 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +

1) Please don't provide handwrittren solution...