The weak base NH3 (concentration 0,10 mol∙dm–3) is titrated with strong acid HCl (concentration 0,050 mol∙dm–3). Without doing any calculations, explain why the pH at the equivalence point of this titration is less than 7.

Q: 10⁻⁸) with 0.100 M LiOH. a) What is the pH of the solution before any base has been added? b) What…

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Q: When a 28.1 mL sample of a 0.423 M aqueous hydrocyanic acid solution is titrated with a 0.462 M…

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Q: The graph above shows the results of the titration of the 20.mL sample of 0.10MHCl(aq) with…

A: Given: Titration curve of the 20. mL sample of 0.10 M HCl(aq) with 0.10 M NaOH(aq) To identify : The…

Q: Consider the titration of a 40.00 mL sample of aqueous dimethylamine, (CH3)2NH, with 0.170 MM HCl.…

A: The concentration of HCl is 0.170 M. The amount of HCl required for the neutralization of…

Q: A student conducts a titration using NaOH (strong base) as the titrant to determine the…

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Q: 1. A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.125 M NaOH,…

A: Given data: Concentration of NaOH = 0.125 M, Volume of NaOH added = 16.00 mL = 0.016 L, pH after…

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is…

A: Given data,[HA]=0.2M[A-]=0.1MpKa=7.5Molarity of KOH=1MVolume of KOH=50mL0.05LVolume of buffer=1L

Q: The pH at equivalence point during a titration of a weak base with a strong acid would be ○ acidic ○…

A: The pH of a solution is a measure of its acidity or alkalinity. It is defined as the negative…

Q: Calculate the pH of the buffer system made up of 0.19 M NH3 and 0.48 M NH₂Cl. The K of NH³ is 1.8 ×…

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Q: Solutions of sodium acetate and acetic acid are combined in equal volume to produce a buffer.…

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Q: Suppose you have 100 mL of a buffer containing 0.100 M acetic acid and 0.0500 M sodium acetate.…

A: The buffer solution are made from the weak acid and its conjugate base or weak base and its…

Q: You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4). This…

A: Given,  Molarity of weak base, (CH3)2NH = 0.250 M  Volume of (CH3)2NH = 30.00 mL  Base dissociation…

Q: n of few more dr

A: Given:  initial pH is 2.90 titrant increased the pH to 4.15 Abrupt increase in pH to 10.00

Q: In the Kjeldahl nitrogen analysis, the final product is NH4 in HCl solution. It is necessary to…

A: The reaction is as follows.NH4+(aq) + H2O(l) ⇌ NH3(aq) + H3O+ (aq)Kb of NH4cl =1.8×10-5Ka=KaKb     =…

Q: 0.35 moles of a weak acid was dissolved in 50.0 mL of water then titrated with a strong base. 30.0…

A: For weak acid and strong base titration, pH at equivalent point is pH = 7 + 1/2(pKa + log C ) Where,…

Q: 70.0 mL of a 0.15 M weak acid (K₂ = 1.8 x 105 ) is titrated with 10 mL of a 0.50 M strong base.…

A: Neutralization reaction is  HA + B →BH+ + A- 1 mole weak acid is neutralized by 1 mole base.

Q: Calculate the pH at the equivalence point in titrating 0.077 M solutions of each of the following…

A: HCl is a strong acid and NaOH is a strong base. This is the titration of strong acid vs strong base.…

Q: Consider the titration of a 60.0 mL of 0.313 M weak acid HA (Ka = 4.2 x 10-6) with 0.400 M KOH. L L…

A: We have to calculate the pH for the given titration

Q: A 0.0420 L volume of 0.11 M hypobromous acid (HBrO), a weak acid with Ka = 2.8 ✕ 10−9, is titrated…

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Q: A chemistry graduate student is given 125. mL of a 0.30M pyridine (CHN) solution. Pyridine is a weak…

A: The concentration of pyridine = 0.30 MThe Kb for pyridine = Mass of  = ?

Q: A chemistry graduate student is given 250. mL of a 1.20M chloroacetic acid (HCH₂CICO₂) solution.…

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Q: Consider the titration of a 25.0-mL sample of 0.115 M CH3COOH with 0.100 М КОН. Ка СН3СООН %3…

A: At equivalence point, number of moles of acid is equal to number of moles of base.

Q: a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF. The Ka for HF is 7.2×10-4.…

A: The pH of a buffer can be calculated by the following formula. pH=pKa + log[conjugate base][acid]

Q: What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl…

A: The reaction at the equivalence point

Q: A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine…

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Q: Choose the false statement. O The pH of the acetic acid solution at the equivalence point is less…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: 100.0 ml of a solution containing 0.200 M NaNO2 is titrated with 0.100 M HCl. Which of the following…

A: We would check the nature of NaNO2 to determine the range of pH .  At half equivalance point ,…

Q: Calculate pH of a buffer containing 0.10 M NH3 and 0.20 M NH4Cl. (Kb NH3 = 1.8 x 10-5).

A: To find out the pH of buffer solution, we need to use the Henderson-Hasselbach equation. First, we…

Q: A mixture of sodium carbonate (Na2CO3) and sodium bicarbonate (NaHCO3) is dissolved in water and…

A: At first end point Na2CO3 reacts with HCl to form NaHCO3. Na2CO3 + HCl ------> NaHCO3 + NaCl…

Q: A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml…

A: The question is based on the volumetric titration of potassium hydrogen phthalate with sodium…

Q: A student obtains a sample of 0.02500 M acetic acid (CH3COOH, 60.05 g/mole, Ka =1.8 x 10-5). 50.00…

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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.