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- Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.Vinegar (chemical name : acetic acid, CH3COOH) is a weak acid. Consider the ionization of acetic acid in water. CH3COOH(aq) = H*(aq) + CH3COO (aq) Kc=6.80 ×10-4 If the initial concentration of acetic acid is 0.150 M. What is the concentration of hydrogen ions (H*) at equilibrium? O 0.0100 M O 0.0500 M O 0.100 M O 0.500 M
- Identify the reaction for this equilibrium expression. K = [H+]²[SO²-] [H2SO4] ○ H2SO4 (aq) = H+ (aq) + SO²¯ (aq) 2 H+ (aq) + SO²¯ (aq) = H₂SO4 (aq) H2SO4 (aq) + H2O (l) = 2 H+ (aq) + SO²¼¯ (aq) + H₂O (1) H₂SO4 (aq) = 2 H+ (aq) + SO²¯ (aq)Consider the following equilibrium of the weak base ammonia in water (NH3, Kb -1.8 x 10). Apart from the water molecules, what species is present in the highest concentration at equilibrium? Nhi(aq) + H2O) = NH,aq) +HO*(aq) O H₂O' O There are equal amounts of NH3 and NH4 The deprotonated form of the ammonia, NH O The protonated form: NH4 Both OH and NH2. When acetic acid (HC2H3O2) dissolves in water, the following reaction happens: HC,H;O,(aq) H,O (1) + H;O* (aq) + CH;O, (aq) K.= 1.79 x 10-5 Find the concentration of all species when 0.100 M acetic acid is dissolved in water. (You can assume that the value of the change (x) is small in this problem.
- Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K= 1.8 x 10-4. HCOOH(aq) + H,O(1) = HCOO (aq) +H,O*(aq) Calculate the equilibrium concentration of H3O* in a 0.985 Msolution. MConsider the reaction: HC,H;O-(aq) + H2O(1) = H;0*(aq) + C,H;O, (aq) K = 1.8 x 10-5 at 25 °C If a solution initially contains 0.210 M HC,H;O, what is the equilibrium concentration of H30* at 25 °C?Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 CH3 COOH (аq) + H20(1) : H30+(aq) + CH3 COO¯ (aq) K =
- The dissociation of acetic acid, CH,COOH, has an equilibrium constant at 25°C of 1.8 x 10-5. CH,COOH(aq) = CH,COO-(aq) + H*(aq) If the equilibrium concentration of CH,COOH is 0.46 moles in 0.500 L of water and that of CH,CO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H+ for the reaction.For the reaction below, Kc = 1.10 × 10-8. Note Kc is sometimes called K. What is the equilibrium concentration of OH- if the reaction begins with 0.610 M HONH,? HONH2 (aq) + H2O (1) HONH3+ (aq) + OH(aq)A student determines that an aqueous solution that contains 0.254 M sodium acetate and 0.417 M acetic acid, also has a H3O+ concentration of 3.90×10-5 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: CH3COOH(aq) + H2O --- H3O+(aq) + CH3COO-(aq) (1) as is usually done, without the inclusion of water in the expression for K: K = (2) for comparison, with the inclusion of water in the expression for K: K =