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- The reaction Cu(s) + HNO3(ag) Cu(NOsh(ag) + 2 NO:) +2 H;O() is used to dissolve the copper metal Ifa 1.000 g sample of copper is used, and instructions say to use four times as much acid as the required amount, how many mL (to the nearest mL) of 15.0 M nitric acid would be used in the procedure for this sample? Select one: O a 10mL Ob 17ml O c.4mL O d 25ml O e 5mLConsider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]Choose the acid below that would make the most effective buffer for a solution to maintain a pH of 5.00 (aq., 25 oC), given a 0.500 M concentration of it and its conjugate salt. a) propionic acid, Ka = 1.34 x 10–5 b) HN3, Ka = 1.90 x 10–5 c) butanoic acid, Ka = 1.52 x 10–5 d) NH4Cl, Ka = 5.56 x 10–10 e) benzoic acid, Ka = 6.30 x 10–5
- 23. lodide ion (1) is the conjugate base of hydroiodic acid (HI). Why doesn't sodium iodide cause an appreciable increase in the pH of water when it dissolves into Na* and I ions? (a) The Na' is acidic and neutralizes the basicity of I (b) It is a stronger acid than it is a base in water, so Nal actually lowers the pH when dissolved. (c) There are no H₂O* ions present in the solution that could react with I. (d) At least a small amount of HI must be present in order for I to act as a base to raise the pH. (e) HI is a strong acid that reacts completely, which makes I a correspondingly weak base. 24. K, for methylamine (CH3NH₂) is the equilibrium constant for which reaction? (a) CHÍNH, + HO - CHÍNH + HO CH₂NH3 + OH* = CHÍNH + H2O CH₂NH™ + H₂O (b) CH₂NH₂ + H₂O (C) CHÍNH, + HO (d) CH₂NH₂ + OH (e) None of the aboveIf the system CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) is saturated with respect to CaCO3, what will happen to the Ca2+ if the pH of the solution begins to decrease? Explain your answer.21:56 1 Question 21 of 30 Submit A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H;PO. is titrated with a 0.800 M NAOH solution. How many ml of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H3PO. , according to the following balanced chemical equation: НРО, + 3 NaOH > NaзРОд + 3 H20 X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 7.50 3 2 22.5 0.250 72.0 1 67.5 m 1000 0.800 0.001 43.2 6.75 x 104 0.0675 Tap here or pull up for additional resources
- Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 669669 mg of AgCl(s) in 100.0 mL of solution. The KspKsp of AgCl is 1.77×10−101.77×10−10.a.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.1. In this week's practical you will be encountering the following equilibrium reaction between lead (I1) ions and iodide ions: Pb(H2O),2* (aq) + 21 (aq) = Pblz (S) + 4 H2O (I) Say if the following statement about this equilibrium system is true or false: If the Pbl2 (s) is slightly soluble in hot water (but not in cold) it means that the above reaction is ENDOTHERMIC. OA. True OB. False
- 11.An acid-base equilibrium system is created by dissolving 0.15 mol HNO2 in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol NO2 (aq) to this solution? How will pH change (calculate pH before and after the addition. For HNO2 Ka = 4.5 x 104)? How will concentrations of HNO2 and NO2 at equilibrium change?To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should be measured (HCO3-+CO2), this was determined by acidifying the sample and measuring the volume of CO2 released. The concentration of H2CO3 was 28.5 mmol/L, the pH of the blood at 37 ℃ is 7.48 with a pka of 6.10, what is the concentration of HCO3- in mmol/L in the blood? a) 27.36b) 22.77c) 28.50d) 29.60(CH3)2O →BF3(g)⇋BF3(g)+(CH3)2O(g) If you place 1.2 g of the complex in a 61.5 mL flask at 125 ℃, what is the total pressure in the flask at equilibrium? What are the partial pressures of the Lewis Acid, Lewis Base, and the complex? (Given: The value of K (here Kp) for the reaction is 0.17 at 125 ℃.) P(BF3)= P((CH3)2O)= P((CH3)2O→BF3)=