Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Write equations for the following separaions. Indicate any conditions required for the reactions to occur, such as pH 5.
(1) Fe^(2+) and Cr^(3+) ions from Ni^(2+) ion.
(2) Fe^(2+) ion from Cr^(3+) ion.
The pH of a 0.10 M solution of Ni(NO3)2 is 5.0. Calculate the acid ionization constant of Ni(H 2O) 62+(aq).
Calculate the pH of the weak acid HF at equilbrium, if the inital concentration of HF was 0.0340 M. (Ka = 1.45 x 10-5)
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- Calculate the pH of a dihydrogen phosphate/hydrogen phosphate buffer prepared with each of the following concentrations. What do you conclude about the pH of a buffer when equal concentrations of the weak acid and conjugate base are used to prepare it? a. 0.10 M NaH 2PO 4 and 0.10 M Na 2HPO 4b. 1.0 M NaH 2PO 4 and 1.0 M Na 2HPO 4c. 0.50 M NaH 2PO 4 and 0.50 M Na 2HPO 4arrow_forward328 K, the K eq for the reaction 2NO 2 (g) rightleftharpoons N 8 O 4 (g) is 1.5. Calculate the concentration of N_{2}*O_{4} present in equilibrium when [N*O_{2}] = 0.50 .arrow_forwardGiven that K = 2.9 x 109 for the following reaction, Zn2+(aq) + 4 NH3(aq) ⇆ Zn(NH3)42+(aq) what is the value of the equilibrium constant for the reverse reaction?arrow_forward
- Think of an experiment you could perform to determine if the iron(III) thiocyanateformation equilibrium is exothermic or endothermic.Fe3+(aq) + SCN‒(aq) ⇌ Fe(SCN)+2(aq)pale yellow(left) deep red(right)arrow_forwardCalculate the pH of a 0.44M solution of HCN. Ka for HCN = 6.2 x 10-10 4.78 1.65 11.42 9.22arrow_forwardThe hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.arrow_forward
- The text describes zinc hydroxide as an amphoteric hydroxide, so Zn(OH)2 is soluble in basic solution. What is the molar solubility of Zn(OH)2 in 1.00 M NaOH? What is the pH of the equilibrium solution?arrow_forwardCalculate the equilibrium concentration of Ni2+ in a 1.0-M solution [Ni(NH3)6](NO3)2.arrow_forwardThe sodium salt of propionic acid, NaCH3CH2CO2 is used as an antifungal agent by veterinarians. Calculate the equilibrium concentration of H3O+ and OH the pH for a solution of 0.10M NaCH3CH2CO2.arrow_forward
- Aqueous Ammonia Solution (with phenolphthalein) NH3 (aq) + H2O (l) = NH4+1 (aq) + OH-1 (aq) What happens to equilibrium by adding HCl to the solution? The reactants are colorless and products are pink.arrow_forwardCalculate the equilibrium concentration of Ni2+ in a 1.0-M solution [Ni(NH3)6](NO3)2.arrow_forwardCobalt(II) complex ion solution: [Co(H2O)6]+2(aq) + 4Cl-(aq) [CoCl4]-2(aq) + 6H2O(l) Pink Blue 1). When silver nitrate is added the blue color becomes pink. Why is that ? 2. When heat is added , in which direction the equilibrium will shift ? Is this reaction exothermic or endothermic ? 3.What happens when the temperature is lowered in the ice bath ?arrow_forward
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