acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an erlenmeyer, you titrate 50 mL of this acid with 0.103 M NaOH and the phenolphtalein indicator duplo. The volume of NaOH needed to reach the equivalence point in both experiments was 48.96 mL and 49.11 mL. a. Write down the equilibrium reaction of dissolving vinegar in water, then write down the equation that reflects the acidic equilibrium constant! b. Calculate the average volume of NaOH needed to reach the equivalence point! c. Calculate the acidity of the vinegar in this sample!

Q: In a titration experiment, how does the error in the standardization of NaOH affect the accuracy in…

A: The error in the standardization of NaOH leads to error in the determination of the concentration…

Q: The pH of the buffer

A:

Q: in a titration, if the mass of KHP in three experimental solutions are 0.467,0.48, and 0.48 and the…

A: Molarity: The concentration of the solutions is given by the term of molarity and it is given by…

Q: Use an Excel spreadsheet to generate a titration curve for 50.00 mL of 0.0200 M ammonia (K, = 1.76 x…

A: The chemical reaction that occurs during the titration of ammonia with HCl is: NH3+HCl↔NH4Cl

Q: You are going to titrate 29.0 mL of 0.294 M cyanic acid (HCNO) with 0.15 M NaOH. What is the pH of…

A: The balanced equation is  HCNO (aq) + NaOH (aq) ---------> NaCNO (aq) + H2O (aq)

Q: a Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.121 M barbituric…

A: Answer:When conjugate base of weak acid is added in water then it gets hydrolysed to produce OH-…

Q: Above is the titration curve of a weak acid (200 mM acetic acid) and strong acid (0.1 M sodium…

A: Solution to be prepared = Acetic acid                  [Acetic acid] to be…

Q: Starting with 0.750 L of a buffer solution containing 0.30 M benzoic acid (C6H5COOH) and 0.35 M…

A: pH = pKa+ log(A-/HA) pH = 4.20 + log(0.35/0.30)=4.26694 after adding mmol of HCl = MV = 340*0.35 =…

Q: 3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5

A: Since, you have asked multiple question, we will solve the first question for you. If you want any…

Q: Consider the titration of 50.0 mL of 0.250 M propanoic acid (Ka = 1.3 x 10-5, pKa = 4.89) with 0.200…

A:

Q: c) Jack and Helen wish to sketch a weak acid strong base titration curve. Before they can do so,…

A:

Q: A mixture contains initially benzoic acid C6H5CO2(weak acid), Ka = 6.28 x 10^-5, and its…

A: Given data :  Ka of benzoic acid = 6.28 x 10^-5 , concentration of benzoic acid = 0.250 M…

Q: Would a precipitate of silver acetate form if 22.0 mL of 0.100 M AgNO3 were added to 45.0 mL of…

A: We know if Ionic product is more than solubility product then precipitate forms. if ionic…

Q: When 40 mL of benzoic acid (C6H5COOH) and 35 mL of potassium hydroxide were titrated, the pH at the…

A: Benzoic acid is a weak acid when strong acid like KOH reacts with it, before equivalence point it…

Q: When 50.00 mL of 0.1000 M of the weak acid was titrated with 0.1000 M NaOH, which of the following…

A: Here we have to determine the weak acid ( 50 ml of 0.1 M )  which gives steepest slope at equivalent…

Q: Prepare 500 mL 0.1 M acetate buffer, pH = 4.3, from 0.1 M stock solutions of acetic acid and its…

A: pH of a buffer is calculated by the following equation.  pH=pKa + log [base][acid]

Q: Given that Kb(NH3) = 1.80 x 10-5 , determine the mass of NH4Cl which must be added to 2.00 L of…

A: Buffer - A buffer solution is an aqueous solution consisting of a weak acid or base and its…

Q: A Mohr titration of NaCl is done at pH 2. Is there a positive error, negative error, no effect, or…

A: A question based on general chemistry that is to be accomplished.

Q: What is the pH of a saturated solution of Ca(OH)₂? Ca(OH)₂ (s) Ca²+ (aq) + 2 OH- (aq) Ksp = 3.7 x 10…

A: Solubility reaction:- Ca(OH)2(s) -------------> Ca2+(aq)  +  2OH-(aq) Ksp = 3.7×10-6

Q: Consider the titration of 110.0 mL analyte solution containing 0.15 mol L-1 NH3 with 0.10 mol L-1…

A: pKb  = - log Kb            =  - log (1.80  * 10-5 )          = 4.745pKa = 14-pKb       = 14- 4.745…

Q: A chemistry graduate student Is glven 100. mL of a 0.70M trimethylamine ((CH,) N solution.…

A:

Q: Which one of the following indicators would be best to use when titrating 0.1M morphine (Kb = 1.6 ×…

A: pH is a measure of hydrogen ion concentration in solution and it measures acidity or alkalinity of a…

Q: 11-C. Calculate the pH at each point listed for the titration of 100.0 mL of 0.100 M cocaine…

A:

Q: You titrated phosphoric acid H3PO4 (Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, Ka3 = 4.2×10-13) with a strong…

A:

Q: Consider the titration of a 75.00 mL sample of 0.300 MM maleic acid, H2C4H2O4 with 0.280 M KOH. It…

A: Given, Volume of maleic acid = 75.00 mL = 0.075 L    (1mL = 0.001 L) Concentration of maleic acid =…

Q: Consider the titration of 30.0 mL of 0.315 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. How…

A: At halfway point , half moles of base are neutralized by acid , HI .  So, we would calculate moles…

Q: a) How many grams of sodium acetate, NACH3COO (molar mass: 82.0343 g/mol) should be combined with…

A: The answer to the following question is-

Q: In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x…

A:

Q: ind the number of grams of potassium hydroxide KOH that would have to be added to 140 mL of a 0.293…

A: Given data,Molarity of HNO2=0.293MVolume of HNO2=140mL=0.140LKa=6.0×10-4pH=3.45

Q: A student was given a solid containing a mixture of nitrate slats. The sample completely dissolved…

A: The objective of the question is to identify the possible nitrate salts present in the unknown…

Q: Consider the following reaction: Ksp of CaCO3 = 4.9 × 10-9 Ka of HCO3¯= 4.7 × 10-11 CaCO3 (s) +…

A: K for the reaction is; CaCO3s↔Ca2+aq+CO32-aq, Ksp=Ca2+CO32- ...... iCO32-aq+H+aq↔HCO3-aq,…

Q: A 29.9 mL sample of 0.299 M methylamine, CH3NH2, is titrated with 0.331 M hydroiodic acid, HI at 25…

A:

Q: A 25.0-mL volume of 0.040 0 M phosphoric acid was titrated with 0.050 0 M tetramethylammonium…

A:

Q: Give 3 uses of buffer solutons or instances where they are important.

A: What is Buffer Solution? The buffer solution is a solution able to maintain its Hydrogen ion…

Q: 2 of 14 Another student is investigating the change in pH during a titration where sodium hydroxide…

A:

Q: Consider the titration of 100.0 mL of 0.200 M acetic acid (K = 1.8 x 10) by 0.100 M KOH. Calculate…

A: Given that 100 ml acetic acid of 0.200 M.Ka of acid = 1.8 × 10^-5by 0.100 M KOH.

Q: find the pH of the solution obtained from 0.34 grams of HCOONa with 100 ml of 0.1 M HCOOH solution…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: a. Calculate the pH in the titration of 50.0 mL 0.03200 M chloroacetic acid (Ka = 1.36 x 10 ¹) after…

A: Given :-  Volume of Chloroacetic acid, ClCH2COOH = 50.0 mL  Molarity of Chloroacetic acid, ClCH2COOH…

Q: In the potentiometric titration of phosphoric acid, pH readings at the first and second…

A: pH1 = 2.12  pH2 = 7.21 pH = pka  pH = -log[H+]  pka = -log ka. Ka1 = ?  Ka2 = ?

Q: Phosphoric acid is a triprotic acid (K₁1 = 6.9 × 10-³, K₁2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-¹³). To…

A:

Q: How would you create a buffer solution at a pH of your choosing (between pH 4-6) by adding solid…

A: Given: Molarity of acetic acid=0.1 M Volume of acetic acid =50 ml Ka=1.75×10-5 pH=4-6 To find: Mass…

Q: A chemist adds enough of the theoretical ionic compound MX3 to form a saturated solution. She knows…

A: One mole of MX3 will dissociates into 1 mole of M3+ and 3 mol X-. Let the solubility of MX3 be “s”

Q: LA solution is prepared at 25 °C that is initially 0.083 M in chloroacetic acid (HCH,CICO,), a weak…

A:

Q: In the titration of a weak monopotic acid HA (Ka = 1.0 x 106) with NaOH, when the volume of base…

A: Given -> Ka = 1.0 × 10-6 -> Acid is weak monoprotic .

Q: B.) This is the titration curve of a formic acid (a weak acid) and a strong base. Give the name of…

A: Titration is defined as the process of determining the quantity of a substance A by adding substance…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.