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- Write the charge-balance equations for a solution that is a. 0.35 M in HCN. b. 0.24 M in (CH3)2NH. + c. saturated with Ag₂ CO3. + + = + +A buffer solution is made that is 0.355 M in HCN and 0.355 M in KCN. If K, for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH =| Write the net ionic equation for the reaction that occurs when 0.095 mol HNO, is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H;0* instead of Ht) A buffer solution is made that is 0.376 M in HCN and 0.376 M in NaCN. If K, for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.105 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +< A buffer solution that is 0.401 M in HF and 0.401 M in KF has a pH of 3.14. The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to A C The capacity of this buffer for added H₂Ot could be increased by the addition of 0.159 mol
- 10a.Determine the molar solubility (?) of Ag2CO3 in a buffered solution with a pH of 5.887 using the systematic treatment of equilibrium. ?sp(Ag2CO3) = 8.46×10−12; ?a1(H2CO3) = 4.45×10−7; ?a2(H2CO3) = 4.69×10−11. S = ? MA buffer is prepared by mixing 0.15 M Na HPO4 and 0.10 M NaH, PO4. Kg for H3PO4 = 7.5 103 K, for H,PO, = 6.2 x 10 8 K, for HPO,2- = 4.2 x 10°13 1) What is the pH of this buffer? 2) Write the chemical reaction that occurs when NaOH is added to this buffer.
- Use the References to access important values if needed for this question. A buffer solution is made that is 0.482 M in H,S and 0.482 M in NaHS. If K for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH= Write the net ionic equation for the reaction that occurs when 0.141 mol HI is added to 1.00 Lof the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use HO* instead of H*) Retry Entire Group No more group attempts remain Submit AnswerA saturated solution of Pb(OH)2 is filtered and 25.00 mL of this solution is titrated with 0.000050 M HCl at 25°C. The volume required to reach the equivalence point of this solution is 6.70 mL. Calculate the concentration of OH", Pb2* and the Ksp of this saturated solution.Please don't provide hnad writtin solution.....
- A buffer is made up of equal volumes of 0.1 M weak acid (AH) and 0.1 M conjugate base (A minus). The pH of the solution is measured to be 4.6. What is the pk, of this weak acid? (HINT: Use the formula pH = pK, + log(Vol A minus/ Vol HA)) %3D O 2.6 O 1.6 O 5.6 O 3.6 O 4.6A chemistry graduate student is given 450. mL of a 1.80M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K= 1.1 × 10 . What mass of KC1O, should the student dissolve in the HC1O, solution to turn it into a buffer with pH = 1.92? You may assume that the volume of the solution doesn't change when the KCIO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.Calculating the composition of a buffer of a given pH Main Menu 0/5 == A chemistry graduate student is given 300. mL of a 1.20M nitrous acid (HNO2) solution. Nitrous acid is a weak acid with K = 4.5 × 10. What mass of KNO, should the student dissolve in the HNO₂ solution to turn it into a buffer with pH = 3.38? You may assume that the volume of the solution doesn't change when the KNO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ ☐ x10 D.P 5