Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. NiS(s)-->
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Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow.
NiS(s)-->
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- Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. HCIO,(aq) – 4- 2- n2+ 3+ D 4+ + 1 3 4 6. 7 8 Os O8 (s) (1) (g) (aq) NR CI Reset • x H,O Delete x H̟O 2 11 3. 2. +Explain how you would separate benzoic acid from NaCl in aqueous solution. Include relevant qualitative test(s) in your explanation.At 77°C, 2.00 mol of notrosyl bromide, NOBr, placed in a 1.00-L flask dissociates to the extent of (9.50x10^0)%; that is, for each mole of NOBr before reaction, (1.000-((9.50x10^0)/100)) mol NOBr remains after dissociation. Calculate the value f Kc for the dissociation reaction 2NOBr(g) ↔ 2NO(g) + Br2(g) Express your answer to three significant figures.
- Calculate the ratio of dissolved benzoic acid to benzoate ion that will exist in solution at equilibrium at a pH of 2.00. The acid equilibrium constant (K a ) for benzoic acid is 6.46 * 10 ^ (- 5) . Note that this calculation doesn't account for the benzoic acid that has precipitated from solution, but you can assume that the higher the ratio, the more benzoic acid will precipitate. Then, Carry out the same calculation for a pH of 4.00, and explain why it was important to reduce the pH to below 4 in this experiment.Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. 9 X Mg(OH)2(s) → > Co the balanced dissociation eq for the com und below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. 10 L C6H3O2(1) – >The value of K, for ethylamine, C,H;NH, is 4.30×104. Write the equation for the reaction that goes with this equilibrium constant. + It is not necessary to include states such as (ag) or (1). +
- Calculate the [H+] and the pH of a buffer solution that is 0.20 M in HC2H3O2 and contains sufficient sodium acetate to make the [C2H3O-2 ] equal to 0.10 M. ( Ka for HC2H3O2 = 1.8 * 10-5)Yeni... O Ara Posta Gonderileri Gözden Geçir Görünüm Yardim 4- Write equations for the acid base reactions that would occur (if any) if ethanol were added to solutions of each of the following compounds In each reaction, label the stronger acid, the stronger base, and so forth.(Please consult the table given below) Ya) NaNH (c) (d) NaOH EGO 16 A 12 IA 17 & 5 8 K(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
- Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH3 CH;NH2 C2H§NH2 CgH;NH2 C3H;N NH,+ CH;NH3* CH;NH3* CH;NH;* C3H;NH+ 1.8 × 10-5 4.38 × 10–4 5.6 × 10-4 3.8 × 10-10 Ammonia Methylamine Ethylamine Aniline Pyridine 1.7 x 10-9 3. Compute the concentration of the weak base in Molarity. (Write your answer in 4 decimal places without the unit).Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).9) a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; + H;O* H¿CO; + H2O (aqueous solution) b) Phenol (HC&H50) is a weak acid (Ka= 1.5 x 10*). Write the equilibrium chemical equation, equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol. 10) Blood is mainly buffered by HCO; /H2CO; (H2CO3, Carbonic Acid, K= 4.4x10 -") buffer system. Calculate the pH of human blood for a carbonic acid concentration of 0.091M and HCO; concentration of 1.00M.