Determine whether a 0.1M solution formed from each of the following salts would be acid, basic, or neutral. NaNO3  NH4Cl KNO2  NH4HCO3  NaHS   

  Determine whether a 0.1M solution formed from each of the following salts would be acid, basic, or neutral. KCl  NaCN CH3NH3I  NH4ClO  NaHCO3   

What is the pH of a 0.025 M CH3COONa solution? Express using 2 decimal places.

A solution contains 0.002 M CO32− and 0.002 M OH−. Choose an answer that fulfills the two following questions when Co(NO3)2 is added slowly to the solution above. Ksp(CoCO3) = 1.0×10−13 and Ksp(Co(OH)2) = 1.0×10−15 Which salt will precipitate first AND what concentration of Co(NO3)2 added will cause its precipitation?  

Consider the following curve for the titration of a weak monoprotic acid (HA) with a strong base and answer each of the following questions: If the question asks for a volume, express your answer in increments of 5 mL (ex: 0, 5, 10, etc.). For all other questions, express your as a whole numbers (1, 2, 3, etc). A. What is the pH at the equivalence point? B. What is the volume of added base at the equivalence point? mL C. At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and Ka of the weak acid? mL D. At what volume of added base does pH=pKa? mL E. What is the pKa of the acid?

In the compound K2 the oxidation number and coordination number of Magnesium are and respectively.

Consider the complex ion 3–. Which of the following responses includes all of the true statements with respect to this complex ion and the ions from which it was formed, and no false statements? I. The complex ion is octahedral. II. Mn3+ is a d5 ion. III. CN– is a strong field ligand. IV. CN– is a weak field ligand. V. The complex ion is a low spin complex. VI. The complex ion is a high spin complex. VII. The complex ion is diamagnetic VIII. The complex ion is paramagnetic

A solution is prepared by adding 0.10 mol of Cobalt (II) Sulfate, CoSO4, to 1.00 L of water. Which statement about the solution is correct?

A buffer with highest capacity can be achieved when pH is equal to the pKa of its acid component. Consider a buffer solution prepared by adding 0.100 M HCl to mL of 0.020 M ammonia. At which volume of hydrochloric acid added will the buffer subsequently achieve its highest buffer capacity? Express your answer to 1 decimal place.

What is the pH of 0.50 M aqueous ethylamine (CH3CH2NH2)? (Kb of CH3CH2NH2= 4.3 x 10–4)