MCQOPTIONS
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MCQOPTIONS
This section includes 11242 Mcqs, each offering curated multiple-choice questions to sharpen your Joint Entrance Exam - Main (JEE Main) knowledge and support exam preparation. Choose a topic below to get started.
| 4851. |
If the pH of a solution of an alkali metal hydroxide is 13.6, the concentration of hydroxide is [JIPMER 2000] |
| A. | Between 0.1 M and 1 M |
| B. | More than 1 M |
| C. | Less than 0.001 M |
| D. | Between 0.01 M and 1 M |
| Answer» B. More than 1 M | |
| 4852. |
One weak acid (like\[C{{H}_{3}}COOH\]) and its strong base together with salt (like \[C{{H}_{3}}COONa\]) is a buffer solution. In which pair this type of characteristic is found [AIIMS 1982; CPMT 1994; MP PET 1994] |
| A. | \[pH\] and \[NaCl\] |
| B. | \[NaOH\] and \[NaN{{O}_{3}}\] |
| C. | \[KOH\] and \[KCl\] |
| D. | \[N{{H}_{4}}OH\] and \[N{{H}_{4}}Cl\] |
| Answer» E. | |
| 4853. |
Which solution has the highest pH value [JIPMER 2000] |
| A. | \[1\,M\,KOH\] |
| B. | \[1\,M\,{{H}_{2}}S{{O}_{4}}\] |
| C. | Chlorine water |
| D. | Water containing carbon dioxide |
| Answer» B. \[1\,M\,{{H}_{2}}S{{O}_{4}}\] | |
| 4854. |
The ionization constant of a certain weak acid is \[{{10}^{-4}}\]. What should be the [salt] to [acid] ratio if we have to prepare a buffer with pH = 5 using this acid and one of the salts [CPMT 2000; KCET 2000; Pb. CET 2000] |
| A. | \[1:10\] |
| B. | \[10:1\] |
| C. | \[5:4\] |
| D. | \[4:5\] |
| Answer» C. \[5:4\] | |
| 4855. |
A buffer solution with \[pH\]9 is to be prepared by mixing \[N{{H}_{4}}Cl\] and \[N{{H}_{4}}OH\]. Calculate the number of moles of \[N{{H}_{4}}Cl\] that should be added to one litre of \[1.0\,M\ N{{H}_{4}}OH.\,\] \[[{{K}_{b}}=1.8\times {{10}^{-5}}]\] [UPSEAT 2001] |
| A. | 3.4 |
| B. | 2.6 |
| C. | 1.5 |
| D. | 1.8 |
| Answer» E. | |
| 4856. |
The condition for minimum change in \[pH\] for a buffer solution is [RPMT 2000] |
| A. | Isoelectronic species are added |
| B. | Conjugate acid or base is added |
| C. | \[pH=p{{K}_{a}}\] |
| D. | None of these |
| Answer» D. None of these | |
| 4857. |
Which would decrease the \[pH\] of \[25\,c{{m}^{3}}\] of a \[0.01\,M\] solution of hydrochloric acid [MH CET 2001] |
| A. | The addition of \[25\,c{{m}^{3}}\] \[0.005\,M\] hydrochloric acid |
| B. | The addition of \[25\,c{{m}^{3}}\] of \[0.02\,M\] hydrochloric acid |
| C. | The addition of magnesium metal |
| D. | None of these |
| Answer» E. | |
| 4858. |
A solution of sodium chloride in contact with atmosphere has a \[pH\]of about [NCERT 1972, 77] |
| A. | 3.5 |
| B. | 5 |
| C. | 7 |
| D. | 1.4 |
| Answer» D. 1.4 | |
| 4859. |
\[pH\] of \[NaCl\]solution is [CET Pune 1998] |
| A. | 7 |
| B. | Zero |
| C. | \[>7\] |
| D. | \[<7\] |
| Answer» B. Zero | |
| 4860. |
The \[p{{K}_{a}}\] of equimolecular sodium acetate and acetic acid mixture is 4.74. If \[pH\] is [DPMT 2001] |
| A. | 7 |
| B. | 9.2 |
| C. | 4.74 |
| D. | 14 |
| Answer» D. 14 | |
| 4861. |
Which buffer solution out of the following will have \[pH>7\] [MP PET 2001] |
| A. | \[C{{H}_{3}}COOH+C{{H}_{3}}COONa\] |
| B. | \[HCOOH+HCOOK\] |
| C. | \[C{{H}_{3}}COON{{H}_{4}}\] |
| D. | \[N{{H}_{4}}OH+N{{H}_{4}}Cl\] |
| Answer» E. | |
| 4862. |
The dissociation constant of HCN is \[5\times {{10}^{-10}}\]. The \[pH\] of the solution prepared by mixing 1.5 mole of HCN and 0.15 moles of KCN in water and making up the total volume to \[0.5\,d{{m}^{3}}\] is [JIPMER 2001] |
| A. | 7.302 |
| B. | 9.302 |
| C. | 8.302 |
| D. | 10.302 |
| Answer» D. 10.302 | |
| 4863. |
A certain buffer solution contains equal concentration of \[{{X}^{-}}\] and \[HX\]. The \[{{K}_{a}}\] for HX is \[{{10}^{-8}}\]. The \[pH\] of the buffer is [UPSEAT 2001] |
| A. | 3 |
| B. | 8 |
| C. | 11 |
| D. | 14 |
| Answer» C. 11 | |
| 4864. |
At \[25{}^\circ C\] the \[pH\] value of a solution is 6. The solution is [AFMC 2001] |
| A. | Basic |
| B. | Acidic |
| C. | Neutral |
| D. | Both B and C |
| Answer» C. Neutral | |
| 4865. |
If \[pH\]of \[A,\,\,B,\,\,C\]and \[D\]are 9.5, 2.5, 3.5 and 5.5 respectively, then strongest acid is [AFMC 1995] |
| A. | A |
| B. | C |
| C. | D |
| D. | B |
| Answer» E. | |
| 4866. |
A solution of sodium borate has a \[pH\] of approximately [JIPMER 2001] |
| A. | < 7 |
| B. | > 7 |
| C. | = 7 |
| D. | Between 4 to 5 |
| Answer» C. = 7 | |
| 4867. |
\[pH\] value of \[N/10\,\,NaOH\] solution is [CBSE PMT 1996;Pb. CET 2001; Pb. PMT 2002] |
| A. | 10 |
| B. | 11 |
| C. | 12 |
| D. | 13 |
| Answer» E. | |
| 4868. |
The addition of solid sodium carbonate to pure water causes [NCERT 1973] |
| A. | An increase in hydronium ion concentration |
| B. | An increase in alkalinity |
| C. | No change in acidity |
| D. | A decrease in hydroxide ion concentration |
| Answer» C. No change in acidity | |
| 4869. |
If the dissociation constant of an acid HA is \[1\times {{10}^{-5}},\] the \[pH\] of a 0.1 molar solution of the acid will be approximately [NCERT 1979] |
| A. | Three |
| B. | Five |
| C. | One |
| D. | Six |
| Answer» B. Five | |
| 4870. |
Out of the following, which pair of solutions is not a buffer solution |
| A. | \[N{{H}_{4}}Cl+N{{H}_{4}}OH\] |
| B. | \[NaCl+NaOH\] |
| C. | \[N{{a}_{2}}HP{{O}_{4}}+N{{a}_{3}}P{{O}_{4}}\] |
| D. | \[C{{H}_{3}}COOH+C{{H}_{3}}COONa\] |
| Answer» C. \[N{{a}_{2}}HP{{O}_{4}}+N{{a}_{3}}P{{O}_{4}}\] | |
| 4871. |
Given a 0.1M solution of each of the following. Which solution has the lowest \[pH\] [MNR 1987] |
| A. | \[NaHS{{O}_{4}}\] |
| B. | \[N{{H}_{4}}Cl\] |
| C. | \[HCl\] |
| D. | \[N{{H}_{3}}\] |
| Answer» D. \[N{{H}_{3}}\] | |
| 4872. |
Which salt can be classified as an acid salt [CPMT 1989] |
| A. | \[N{{a}_{2}}S{{O}_{4}}\] |
| B. | \[BiOCl\] |
| C. | \[Pb(OH)Cl\] |
| D. | \[N{{a}_{2}}HP{{O}_{4}}\] |
| Answer» E. | |
| 4873. |
The \[pH\] of 0.001 molar solution of \[HCl\] will be [MP PET 1986; MP PET/PMT 1988; CBSE PMT 1991] |
| A. | 0.001 |
| B. | 3 |
| C. | 2 |
| D. | 6 |
| Answer» C. 2 | |
| 4874. |
When \[{{10}^{-8}}\]mole of \[HCl\] is dissolved in one litre of water, the \[pH\]of the solution will be [CPMT 1973, 94; DPMT 1982] |
| A. | 8 |
| B. | 7 |
| C. | Above 8 |
| D. | Below 7 |
| Answer» E. | |
| 4875. |
The \[pH\] of the solution containing 10 \[ml\]of 0.1 N \[NaOH\] and 10 \[ml\] of 0.05 N \[{{H}_{2}}S{{O}_{4}}\] would be [CPMT 1987; Pb. PMT 2002,04] |
| A. | 0 |
| B. | 1 |
| C. | > 7 |
| D. | 7 |
| Answer» C. > 7 | |
| 4876. |
The \[pH\]of a solution is the negative logarithm to the base 10 of its hydrogen ion concentration in [Manipal MEE 1995] |
| A. | Moles per litre |
| B. | Millimoles per litre |
| C. | Micromoles per litre |
| D. | Nanomoles per litre |
| Answer» B. Millimoles per litre | |
| 4877. |
The \[{{H}^{+}}\]ion concentration is \[1.0\times {{10}^{-6}}\] mole/litre in a solution. Its pH value will be [MP PMT 1985; AFMC 1982] |
| A. | 12 |
| B. | 6 |
| C. | 18 |
| D. | 24 |
| Answer» C. 18 | |
| 4878. |
The \[pH\] of a \[{{10}^{-10}}\] molar \[HCl\] solution is approximately [NCERT 1977] |
| A. | 10 |
| B. | 7 |
| C. | 1 |
| D. | 14 |
| Answer» C. 1 | |
| 4879. |
Which is a buffer solution [CPMT 1985, 88; AIIMS 1980; MP PMT 1994; AFMC 2004] |
| A. | \[C{{H}_{3}}COOH+C{{H}_{3}}COONa\] |
| B. | \[C{{H}_{3}}COOH+C{{H}_{3}}COON{{H}_{4}}\] |
| C. | \[C{{H}_{3}}COOH+N{{H}_{4}}Cl\] |
| D. | \[NaOH+NaCl\] |
| Answer» B. \[C{{H}_{3}}COOH+C{{H}_{3}}COON{{H}_{4}}\] | |
| 4880. |
\[{{10}^{-6}}M\,\,HCl\] is diluted to 100 times. Its \[pH\]is [CPMT 1984] |
| A. | 6.0 |
| B. | 8.0 |
| C. | 6.95 |
| D. | 9.5 |
| Answer» D. 9.5 | |
| 4881. |
The \[pH\] of \[\frac{N}{100}\]HCl would be approximately [CPMT 1971; DPMT 1982, 83; MP PMT 1991; Bihar MEE 1996] |
| A. | 1 |
| B. | 1.5 |
| C. | 2 |
| D. | 2.5 |
| Answer» D. 2.5 | |
| 4882. |
The hydrogen ion concentration in a given solution is \[6\times {{10}^{-4}}.\] Its \[pH\] will be [EAMCET 1978] |
| A. | 6 |
| B. | 4 |
| C. | 3.22 |
| D. | 2 |
| Answer» D. 2 | |
| 4883. |
As the temperature increases, the \[pH\] of a \[KOH\] solution [UPSEAT 2001] |
| A. | Will decreases |
| B. | Will increases |
| C. | Remains constant |
| D. | Depends upon concentration of \[KOH\] solution |
| Answer» B. Will increases | |
| 4884. |
The pH of \[{{10}^{-8}}\]molar aqueous solution of \[HCl\]is [CPMT 1988; MNR 1983, 90; MP PMT 1987; IIT 1981; BHU 1995; AFMC 1998; MP PET 1989, 99; BCECE 2005] |
| A. | \[-8\] |
| B. | 8 |
| C. | \[6>7\] (Between 6 and 7) |
| D. | \[7>8\] (Between 7 and 8) |
| Answer» D. \[7>8\] (Between 7 and 8) | |
| 4885. |
Assuming complete ionisation, the \[pH\] of \[0.1\,M\,\,HCl\]is 1. The molarity of \[{{H}_{2}}S{{O}_{4}}\] with the same \[pH\] is [KCET 1998] |
| A. | 0.2 |
| B. | 0.1 |
| C. | 2.0 |
| D. | 0.05 |
| Answer» E. | |
| 4886. |
Which of the following solutions cannot act as a buffer [EAMCET 1998] |
| A. | \[Na{{H}_{2}}P{{O}_{4}}+{{H}_{3}}P{{O}_{4}}\] |
| B. | \[C{{H}_{3}}COOH+C{{H}_{3}}COONa\] |
| C. | \[HCl+N{{H}_{4}}Cl\] |
| D. | \[{{H}_{3}}P{{O}_{4}}+N{{a}_{2}}HP{{O}_{4}}\] |
| Answer» D. \[{{H}_{3}}P{{O}_{4}}+N{{a}_{2}}HP{{O}_{4}}\] | |
| 4887. |
The \[pH\]of a solution is 2. If its \[pH\] is to be raised to 4, then the \[[{{H}^{+}}]\] of the original solution has to be [MP PET 1994] |
| A. | Doubled |
| B. | Halved |
| C. | Increased hundred times |
| D. | Decreased hundred times |
| Answer» E. | |
| 4888. |
Aqueous solution of \[HCl\] has the \[pH=4\]. Its molarity would be [RPMT 1999] |
| A. | 4 M |
| B. | 0.4 M |
| C. | 0.0001 M |
| D. | 10 M |
| Answer» D. 10 M | |
| 4889. |
Pure water is kept in a vessel and it remains exposed to atmospheric \[C{{O}_{2}}\]which is absorbed, then its pH will be [MADT Bihar 1984; DPMT 2002] |
| A. | Greater than 7 |
| B. | Less than 7 |
| C. | 7 |
| D. | Depends on ionic product of water |
| Answer» C. 7 | |
| 4890. |
The \[pH\]of a solution is increased from 3 to 6. Its \[{{H}^{+}}\]ion concentration will be [EAMCET 1998] |
| A. | Reduced to half |
| B. | Doubled |
| C. | Reduced by 1000 times |
| D. | Increased by 1000 times |
| Answer» D. Increased by 1000 times | |
| 4891. |
A base is dissolved in water yields a solution with a hydroxide ion concentration of 0.05 \[mol\,\,litr{{e}^{-1}}.\] The solution is [AFMC 1997] |
| A. | Basic |
| B. | Acid |
| C. | Neutral |
| D. | Both A and B |
| Answer» B. Acid | |
| 4892. |
The concentration of hydronium \[({{H}_{3}}{{O}^{+}})\] ion in water is [CET Pune 1998] |
| A. | Zero |
| B. | \[1\times {{10}^{7}}\,gm\,\,ion/litre\] |
| C. | \[1\times {{10}^{-14}}\,gm\,\,ion/litre\] |
| D. | \[1\times {{10}^{-7}}\,gm\,\,ion/litre\] |
| Answer» E. | |
| 4893. |
When the \[pH\]of a solution is 2, the hydrogen ion concentration in moles per litre is [NCERT 1973; MNR 1979] |
| A. | \[1\times {{10}^{-14}}\] |
| B. | \[1\times {{10}^{-2}}\] |
| C. | \[1\times {{10}^{-7}}\] |
| D. | \[pH\] |
| Answer» C. \[1\times {{10}^{-7}}\] | |
| 4894. |
In a solution of acid \[{{H}^{+}}\]concentration is \[{{10}^{-10}}M.\] The pH of this solution will be |
| A. | 8 |
| B. | 6 |
| C. | Between 6 and 7 |
| D. | Between 3 and 6 |
| Answer» D. Between 3 and 6 | |
| 4895. |
An aqueous solution whose \[O{{H}^{-}}\] is [CPMT 1976; DPMT 1982] |
| A. | Alkaline |
| B. | Acidic |
| C. | Neutral |
| D. | Amphoteric |
| Answer» C. Neutral | |
| 4896. |
If the \[pH\] of a solution is 4.0 at \[{{25}^{o}}C,\] its \[pOH\] would be \[({{K}_{w}}={{10}^{-14}})\] [MP PMT 1989] |
| A. | 4.0 |
| B. | 6.0 |
| C. | 8.0 |
| D. | 10.0 |
| Answer» E. | |
| 4897. |
A buffer solution is a mixture of [MP PMT 1987] |
| A. | Strong acid and strong base |
| B. | Weak acid and weak base |
| C. | Weak acid and conjugate acid |
| D. | Weak acid and conjugate base |
| Answer» E. | |
| 4898. |
At 25°C, the dissociation constant of a base BOH is \[1.0\times {{10}^{-12}}\]. The concentration of Hydroxyl ions in 0.01 M aqueous solution of the base would be [CBSE PMT 2005] |
| A. | \[2.0\times {{10}^{-6}}mol\,{{L}^{-1}}\] |
| B. | \[1.0\times {{10}^{-5}}mol\ {{L}^{-1}}\] |
| C. | \[1.0\times {{10}^{-6}}mol\,{{L}^{-1}}\] |
| D. | \[1.0\times {{10}^{-7}}mol\ {{L}^{-1}}\] |
| Answer» E. | |
| 4899. |
\[pH\]of 0.005 \[M\,\,{{H}_{2}}S{{O}_{4}}\] solution will be [NCERT 1980] |
| A. | 0.005 |
| B. | 2 |
| C. | 1 |
| D. | 0.01 |
| Answer» C. 1 | |
| 4900. |
Which of the following is not a Bronsted acid [BHU 1997] |
| A. | \[C{{H}_{3}}NH_{4}^{+}\] |
| B. | \[C{{H}_{3}}CO{{O}^{-}}\] |
| C. | \[{{H}_{2}}O\] |
| D. | \[HSO_{4}^{-}\] |
| Answer» C. \[{{H}_{2}}O\] | |