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Acids, bases and buffers

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Question 2

40.0 cm3 of 0.250 mol dm−3 HNO30.250\text{ mol dm}^{-3}\ \text{HNO}_30.250 mol dm−3 HNO3​ is added to 60.0 cm3 of 0.100 mol dm−3 KOH0.100\text{ mol dm}^{-3}\ \text{KOH}0.100 mol dm−3 KOH.

What is the concentration of the resulting solution?

0.0400 mol dm−3 HNO30.0400\text{ mol dm}^{-3}\ \text{HNO}_30.0400 mol dm−3 HNO3​ and 0.0400 mol dm−3 KNO30.0400\text{ mol dm}^{-3}\ \text{KNO}_30.0400 mol dm−3 KNO3​

0.0400 mol dm−3 HNO30.0400\text{ mol dm}^{-3}\ \text{HNO}_30.0400 mol dm−3 HNO3​ and 0.0600 mol dm−3 KNO30.0600\text{ mol dm}^{-3}\ \text{KNO}_30.0600 mol dm−3 KNO3​

0.0600 mol dm−3 HNO30.0600\text{ mol dm}^{-3}\ \text{HNO}_30.0600 mol dm−3 HNO3​ and 0.0400 mol dm−3 KNO30.0400\text{ mol dm}^{-3}\ \text{KNO}_30.0400 mol dm−3 KNO3​

0.100 mol dm−3 HNO30.100\text{ mol dm}^{-3}\ \text{HNO}_30.100 mol dm−3 HNO3​ and 0.0600 mol dm−3 KNO30.0600\text{ mol dm}^{-3}\ \text{KNO}_30.0600 mol dm−3 KNO3​

Acids, bases and buffers Questions

  1. A Level
  2. /Chemistry
  3. /Acids, bases and buffers