Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated form is yellow.  What is the color if this indicator in a solution with pH = 3.7? yellow green red orange blu

Q: A weak acid has Ka of 4.47 x 10-4.  What is pKa for this weak acid?

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Q: buffer of pH = 7.5 is desired. Which two of the following compounds should be dissolved in water in…

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

Q: Consider the buffer system of ammonia, NH3 and ammonium ion NH4+ (Ka= 5.6 x10^-10)  a) what is the…

A: Value of pH of a solution is used to measure the acidity or basicity of a solution. At room…

Q: Buffer solutions are used by the human body to maintain a constant pH for biochemical processes such…

A: pH and ratios of concentration of conjugate base and weak acid concentration from the Henderson…

Q: The indicator bromothymol blue is yellow in a solution whose pH is less than 6.0, green if the pH of…

A: Given--<>  [H3O+] = 3.45 ×10-3 M what is color of bromothymol blue = ?

Q: The table below shows the plH values at which two different indicators change colour Indicator…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub- parts for…

Q: What is the pH of 0.1 M HCN solution? (K, for HCN = 6.2 × 10-10) А. 1.5 В. 1.0 С. 5.1 D. 8.9 Е. 7.5…

A: pH of a solution = - log [H+] where [H+] is the concentration of H+] in the solution At…

Q: 2. The weak acid hypochlorous acid (HClO) is formed in bleach solutions. If the pH of a 0.12 M…

A: In multiplart questions we solve only three subquestion according to Bartleby Guidelines. pH of any…

Q: A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough…

A: Buffer solution is the solution which has tendency to maintain constant pH upon addition of small…

Q: What is the pH of a buffer solution that is 0.251 mol L in lactic acid and 0.151 mol L in sodium…

A: Given: Concentration of Lactic Acid= 0.251 mol L-1 Concentraion of Sodium Lactate= 0.151 mol L-1 Ka=…

Q: The indicator ethyl orange is an acid with a Ka of 4.6 ✕ 10−5. In a 1.9 ✕ 10−4 M solution, it is red…

A: The change in color of ethyl orange, when the pH of solution is changed, shown below.

Q: A 25.00 mL sample of methanoic (HCHO2, Ka = 1.8 x 10-4) is titrated to the equivalence point using…

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Q: A buffer solution is made that is 0.440 M in HClO and 0.440 M in NaClO. (1) If Ka for HClO is…

A: Given : Concentration of weak acid HClO = 0.440 M And concentration of conjugate base salt of weak…

Q: You want a buffer solution, and you choose the following acid and conjugate base: carbonic acid,…

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Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: Given : Ka = 2 x 10-4  thymol orange is an acidic indicator.

Q: An indicator (Ka = 1.7X10-6) is red but changes to blue when ionized. The indicator was used in the…

A: The pH range of the indicator is 4.77 - 6.77. So the correct option is option E.

Q: What is the pH of a buffer solution that contains 0.25 M HClO and 0.35 M NaClO? (pKa HClO = 7.46)…

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Q: An analytical chemist is titrating 160.2 mL of a 0.3300M solution of nitrous acid (HNO,) with a…

A: Given: The reaction is as follows: HNO2(g) + KOH(l)   ⇌  KNO2(aq) + H2O.  The volume of HNO2, (V1) =…

Q: mixture of solid chloride salts known to contain only some of the cations of Experiment 12 is…

A: Precipitation is process  transforming a dissolved  substance  into an  insoluble  solid.  The…

Q: There is a buffer solution containing 0.50 M acetic acid (CH3COOH, Ka= 1.8 X 10-5) and 0.50 M sodium…

A: A buffer is used to maintain the pH of the solution when the addition of acid or base is done. pH of…

Q: Calculate the pH of a buffer that is 0.040 M HA and 0.020 M NaA.  HA is a weak acid and its K a is…

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Q: A monoprotic weak acid, HAHA, dissociates in water according to the reaction…

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Q: Which of the following aqueous solutions are good buffer systems? O 0.14 M hypochlorous acid + 0.18…

A: Buffer solution is combination of weak acid or base with salt of weak acid or base respectively.

Q: a. What quantity (moles) of NaOH must be added to 1.0 L of 1.7 M HC, H3O2 to produce a solution…

A: Here we have to determine the moles of NaOH should be added to 1Liter of 1.7 M CH3COOH to make the…

Q: Which of the following is more likely to precipitate the hydorxide ion? (a) Cu(OH)2(s) = Cu2+(aq) +…

A: Actually, the molar solubility is the amount of solutes that can be dissolved in per liter of…

Q: Magnesium hydroxide, Mg(OH). has a K of approximately 5.61x10-12 Part A Calculate the molar…

A: Given that:  Ksp of Mg(OH)2 = 5.61×10-12 pH = 8.57 pH + pOH = 14 pOH = 14- pH = 14 - 8.57 = 5.43…

Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

A: Buffer solution - A solution whose pH is not altered to any great extent by the addition of small…

Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 8.95? K„ (Mg(OH)2) = 1.8…

A: Concentration of OH- can be calculated as follows:

Q: Calculate the pH of a dihydrogen phosphate/hydrogen phosphate buffer prepared with each of the…

A: The pH of a buffer can be calculated by using the Henderson-Hassalablch equation. The formula is:…

Q: A certain indicator, HA, has a K₂ value of 4.0 x 10-6. The protonated form of the indicator is red…

A: Given data :  Ka=4.0×10-6pH=7 To find: pKa and color of indicator at pH 7

Q: Which of the following weak acids when paired with its conjugate base would be the best choice for a…

A: Given group of answer choices : a). HClO: pKa = 7.54 b). C5H4NH+: pKa = 5.25 c). HNO2: pKa =…

Q: In the titration of 100.0 mL of 0.050 M HClO2 (pKa = 1.96)  solution with a 0.10 M NaOH titrant,…

A: Given: Concentration of HClO2 = 0.050 M Volume of HClO2 solution = 100.0 mL = 0.100 L…

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

A:

Q: A 200mL solution of 0.3 M weak acid is titrated with 40 mL of 1.5 M NaOH. If the Ka of the acid is…

A: Number of mmoles of HA = Molarity x volume (mL) = 0.3 x 200 = 60 mmoles Number of moles of NaOH =…

Q: 0.0158 M LiClO and 0.099 M HClO in 2.5 L.  The ka of HClO = 2.9e-8.

A: Given data are as follows: LiClO concentration=0.0158 M  HClO concentration=0.099 M ka of HClO =…

Q: The following reaction occurs: HNO,(aq) + NaOH(aq) → NaNO,(aq) + 2 H,0(1) Identify the correct…

A: When strong acid react with strong base neutralization takes place. (NaNO3 neutral salt) At…

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

A:

Q: The pH of buffer solution that has Ka = 6.23 x 105 and 5a, = 3a, is: а. 4.43 b. 4.03 С. 4.38 d. 3.98…

A: pH = d.  3.98

Q: Methyl orange is an indicator used for detecting the pH of acidic solutions. The red, protonated…

A:

Q: titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of…

A: We have to find molarity of HCl solution

Q: Buffer solutions are used by the human body to maintain a constant pH for biochemical processes such…

A: Ka = 1.85 × 10-5 [ CH3COOH ] = 0.150 M [ CH3COO- ] = 0.150 M pKa = -logKa

Q: A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M…

A:

Q: Consider the buffer system of ammonia, NH3 and ammonium ion NH4+ (Ka= 5.6 x10^-10)  a) what is the…

A: Solution -

Q: Write the balanced equation when 1 drop of NH4OH, 20 drops of distilled water, 6M of HCI is added…

A: Note - The given data in parts, i.e, a. Co(COH)3, b. Al(OH)3, and so on, has no relevance in the…

Q: Which statement about acid-base indicators is not correct? *       A- A weak acid can be used as an…

A: Acid-base indicators made of weak acids and weak bases. Due to common ion effect.

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

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Q: Lactic acid has a K. of 2.502 x 103. A solution contains 0.275 M lactic acid and 0.375 M sodium…

A: Buffer solution: The mixture of lactic acid and sodium lactate act as a buffer solution. The…

Q: A solution containing 25mL of 0.0750M Maleic acid (diprotic acid) is titrated with 0.05M NaOH.…

A:

Q: An indicator with Ka = 6.45 X 10-5 is yellow in acid and blue in base.   Showing a calculation for…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.